Search found 17642 matches

by Chem_Mod
Sun Aug 21, 2011 12:31 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: How do salts play a role in a buffer?
Replies: 1
Views: 204

Re: How do salts play a role in a buffer?

Answer: Salts work well to buffer the pH of solution because you pick a specific salt wisely. In the generic equation HA --> H+ + A-, you pick your salt to contain the cation A-. Thus, in a solution of this salt and HA, due to the high relative concentrations of HA and A-, the solution is rather ro...
by Chem_Mod
Sun Aug 21, 2011 12:31 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: How do salts play a role in a buffer?
Replies: 1
Views: 204

How do salts play a role in a buffer?

Question: How do salts play a role in a buffer?
by Chem_Mod
Sun Aug 21, 2011 12:29 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: H3PO4 has only one H atom?
Replies: 1
Views: 231

Re: H3PO4 has only one H atom?

Answer: At pH 12 the solution is alkaline and the H3PO4 has already lost 2 or 3 H+ to form Na2HPO4 and Na3PO4. These are the species in solution at pH 12.
by Chem_Mod
Sun Aug 21, 2011 12:29 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: H3PO4 has only one H atom?
Replies: 1
Views: 231

H3PO4 has only one H atom?

Question: When determining the pH values of a buffer, how come the pH value listed for the compound H3PO4 is 12, but the species NaHPO4 added with Na3PO4 also have a pH of 12. Why do these species only have one H atom, instead of 3 in H3PO4.
by Chem_Mod
Sun Aug 21, 2011 12:28 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: How to find volume of solution added using HH equation
Replies: 1
Views: 562

Re: how to find volume of solution added using HH equation

Answer: Using the Henderson-Hasselbalch equation you can determine the ratio of acid to base. This is equal to the ratio of moles of acid and base. Given the known moles of the acid you can then determine the moles of base necessary and calculate the volume necessary to deliver that many moles of b...
by Chem_Mod
Sun Aug 21, 2011 12:27 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: How to find volume of solution added using HH equation
Replies: 1
Views: 562

How to find volume of solution added using HH equation

Question: How can we find the volume of a solution added using the Henderson-Hasselbalch equation?
by Chem_Mod
Sun Aug 21, 2011 12:24 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: What conditions can we use the HH equation?
Replies: 1
Views: 403

Re: what conditions can we use the Henderson equation

Answer: The Henderson-Hasselbalch equation is used under the condition of weak acid and a salt or a weak base and a salt. Both of these are buffer solutions.
by Chem_Mod
Sun Aug 21, 2011 12:23 pm
Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
Topic: What conditions can we use the HH equation?
Replies: 1
Views: 403

What conditions can we use the HH equation?

Question: Under what conditions can we use the Henderson equation to calculate the pH if we're not told in the question that there is a buffer involved? How do we know if a solution contains a buffer or not?
by Chem_Mod
Sun Aug 21, 2011 12:20 pm
Forum: Identifying Acidic & Basic Salts
Topic: KBr is neutral, but why KF is basic?
Replies: 1
Views: 7992

Re: KBr is neutral, but why KF is basic?

F- is an exception in that it is the only halogen that affects the pH of a solution. If one thinks about the series H-F, H--Cl, H---Br, H----I and recalls that H-F is the weakest acid (strongest bond) then it makes sense that F- will pick up H+ from water to form H-F and OH- and hence raise the solu...
by Chem_Mod
Sun Aug 21, 2011 12:20 pm
Forum: Identifying Acidic & Basic Salts
Topic: KBr is neutral, but why KF is basic?
Replies: 1
Views: 7992

KBr is neutral, but why KF is basic?

K+ is not an acid and Br- is not a base, so the solution is neutral. But KF is basic, why is it not also neutral since they both have K+ and Br and F are in the same group? Also for compounds such as AlCl3 and Cu(NO3)2, how do I determine that it is Al(H2O)6 or Cu(H2O)6 when I am writing out the che...
by Chem_Mod
Sun Aug 21, 2011 12:20 pm
Forum: Identifying Acidic & Basic Salts
Topic: How do you write the reaction for NaOH + CH3HOOH?
Replies: 1
Views: 307

Re: How do you write the reaction for NaOH + CH3HOOH?

base + acid ---> salt + water NaOH + CH3COOH -----> CH3COO-Na+ + H2O
by Chem_Mod
Sun Aug 21, 2011 12:19 pm
Forum: Identifying Acidic & Basic Salts
Topic: How do you write the reaction for NaOH + CH3HOOH?
Replies: 1
Views: 307

How do you write the reaction for NaOH + CH3HOOH?

How do you write the reaction for NaOH + CH3HOOH?
by Chem_Mod
Sun Aug 21, 2011 12:18 pm
Forum: Polyprotic Acids & Bases
Topic: H2SO3 and NaOH, how many moles of NaOH are needed to neutral
Replies: 1
Views: 1574

Re: H2SO3 and NaOH, how many moles of NaOH are needed to neu

Because H2SO3 has two protons, 2 hydroxides are required to neutralize it, yielding the 2:1 ratio of NaOH:H2SO3 needed.
by Chem_Mod
Sun Aug 21, 2011 12:18 pm
Forum: Polyprotic Acids & Bases
Topic: H2SO3 and NaOH, how many moles of NaOH are needed to neutral
Replies: 1
Views: 1574

H2SO3 and NaOH, how many moles of NaOH are needed to neutral

For a reaction of H2SO3 and NaOH, how many moles of NaOH are needed to neutralize it?
by Chem_Mod
Sun Aug 21, 2011 12:18 pm
Forum: Polyprotic Acids & Bases
Topic: why use the pKa for H2PO3- not HPO3(2-)?
Replies: 1
Views: 1719

Re: why use the pKa for H2PO3- not HPO3(2-)?

Use the Henderson-Hasselbach equation, pH = pKa + log([base]/[acid]). In the case of these species, H2PO3- + H2O -> HPO3(2-) + H30+, thus the dihydrogen species is the acid, and the monohydrogen specie is the base. Given that, in the Henderson-Hasselbach equation the pKa of dihydrogen phosphate must...
by Chem_Mod
Sun Aug 21, 2011 12:18 pm
Forum: Polyprotic Acids & Bases
Topic: why use the pKa for H2PO3- not HPO3(2-)?
Replies: 1
Views: 1719

why use the pKa for H2PO3- not HPO3(2-)?

How do we differentiate to use the pKa for potassium dihydrogen phosphate and not the pKa for potassium hydrogen phosphate?
by Chem_Mod
Sun Aug 21, 2011 12:16 pm
Forum: Polyprotic Acids & Bases
Topic: How do you find the value for pKa3 for phosphoric acid?
Replies: 1
Views: 1220

Re: How do you find the value for pKa3 for phosphoric acid?

Remember that phosphoric acid is a triprotic acid (H3PO4). Ka1 refers to the reaction that removes the first hydrogen: H3PO4 + H2O <-> H2PO4- + H3O+. Ka2 refers to the reaction that removes the second hydrogen: H2PO4- + H2O <-> HPO4-2 + H3O+. Ka3 refers to removing the last hydrogen: HPO4-2 + H2O <-...
by Chem_Mod
Sun Aug 21, 2011 12:16 pm
Forum: Polyprotic Acids & Bases
Topic: How do you find the value for pKa3 for phosphoric acid?
Replies: 1
Views: 1220

How do you find the value for pKa3 for phosphoric acid?

How do you find the value for pKa3 for phosphoric acid?
by Chem_Mod
Sun Aug 21, 2011 12:15 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: What is the relationship between pKa to the pH or pOH?
Replies: 1
Views: 294

Re: What is the relationship between pKa to the pH or pOH?

Answer: The relationship between pKa and pH is given by the Henderson-Hasselbach equation. Acid strength increases with decreasing pKa. A strong acid is not represented with an equilibrium constant because it is assumed to dissociate completely (Ka is "infinite," if you want). Weak acid d...
by Chem_Mod
Sun Aug 21, 2011 12:15 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: What is the relationship between pKa to the pH or pOH?
Replies: 1
Views: 294

What is the relationship between pKa to the pH or pOH?

Question: Is there any relation between pKa and the pH or pOH? The smaller the pKa, the stronger the acid. The lower the pH, the stronger the acid. But why are certain acids with very small pKa (ex trichloroacetic) still considered weak acids?
by Chem_Mod
Sun Aug 21, 2011 12:15 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: Use KaKb=Kw for strong acid/base, ICE box for weak?
Replies: 1
Views: 691

Re: Use KaKb=Kw for strong acid/base, ICE box for weak?

Answer: When you have strong acids and bases that dissociate completely, you can directly calculate the pH (pOH) without having to do an ICE box. You wouldn't use Ka or Kb for strong acids and bases, respectively, because dissociation is assumed to be 100%.
by Chem_Mod
Sun Aug 21, 2011 12:14 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: Use KaKb=Kw for strong acid/base, ICE box for weak?
Replies: 1
Views: 691

Use KaKb=Kw for strong acid/base, ICE box for weak?

Question: When we calculate the the H3O+ and OH- concentrations for strong acids and bases, can we use KaKb = Kw, because these acids/bases dissociate completely? As opposed to weak acids and bases when we have to use the ICE box?
by Chem_Mod
Sun Aug 21, 2011 12:13 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: How can a solution be neutral if [H3O+] is less than 10-7?
Replies: 1
Views: 347

Re: How can solution be neutral if [H3O+] is less than 10-7?

Answer: Neutral water has 10-7 M H3O+. If one calculates that a compound when added to neutral water produces H3O+ (equivalent to a concentration of 10-10 M H3O+) then the compound is hardly increasing the H3O+concentration above 10-7 M. In other words, add 10-10 M H3O+ + 10-7 M H3O+ and then take ...
by Chem_Mod
Sun Aug 21, 2011 12:13 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: How can a solution be neutral if [H3O+] is less than 10-7?
Replies: 1
Views: 347

How can a solution be neutral if [H3O+] is less than 10-7?

Question: I was confused about the last statement you made at the end of class: "If [H3O+] < 10-7, then the solution is considered neutral because we know that as a result of autoprotolysis they are 10-7 M H3O+." I am have trouble understanding how a solution would be neutral if [H3O+] is...
by Chem_Mod
Sun Aug 21, 2011 12:13 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: What do one arrow and double arrows stand for?
Replies: 1
Views: 7972

Re: what do one arrow and double arrows stand for?

Answer: Correct! Although, all chemical reactions are reversible, so a double arrow is never incorrect.
by Chem_Mod
Sun Aug 21, 2011 12:12 pm
Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
Topic: What do one arrow and double arrows stand for?
Replies: 1
Views: 7972

What do one arrow and double arrows stand for?

Question: For a strong acid and strong base reaction, there is only one arrow representing that all of the reactants are converted to products, right? So, for weak acids and bases that do not dissociate completely, the double arrows are used, right?
by Chem_Mod
Sun Aug 21, 2011 12:11 pm
Forum: Conjugate Acids & Bases
Topic: Ka and Kb able to tell acid/base weak or strong?
Replies: 1
Views: 3385

Re: Ka and Kb able to tell acid/base weak or strong?

Really strong acid/base has a Ka/Kb larger than 1. Although I would consider a strong acid/base with a Ka/Kb larger than 10^-3.
by Chem_Mod
Sun Aug 21, 2011 12:10 pm
Forum: Conjugate Acids & Bases
Topic: Ka and Kb able to tell acid/base weak or strong?
Replies: 1
Views: 3385

Ka and Kb able to tell acid/base weak or strong?

For the section on weak acids and bases, if only Ka or Kb are given, is there a way to tell whether the acid/base will be weak or strong?
by Chem_Mod
Sun Aug 21, 2011 12:09 pm
Forum: Conjugate Acids & Bases
Topic: Clarification for Ka and Kb
Replies: 1
Views: 286

Re: Clarification for Ka and Kb

All your statements are correct.
by Chem_Mod
Sun Aug 21, 2011 12:09 pm
Forum: Conjugate Acids & Bases
Topic: Clarification for Ka and Kb
Replies: 1
Views: 286

Clarification for Ka and Kb

I wanted to clarify the concept of Ka (aciditiy constant) and Kb (basicity constant). We know that when Ka is a large number, such as 10-1, then it is a stronger acid because it has greater [H3O+]. So if Kb is also a large number such as 10-1, then it should also be a stronger base compared to a Kb ...
by Chem_Mod
Sun Aug 21, 2011 12:09 pm
Forum: Conjugate Acids & Bases
Topic: Are all carbonic acids generally considered to be weak?
Replies: 1
Views: 344

Re: Are all carbonic acids generally considered to be weak?

Since carbonic acid, H2CO3 has Ka1 = 4.3 x 10^-7, it is a weak acid.
by Chem_Mod
Sun Aug 21, 2011 12:08 pm
Forum: Conjugate Acids & Bases
Topic: Are all carbonic acids generally considered to be weak?
Replies: 1
Views: 344

Are all carbonic acids generally considered to be weak?

Are all carbonic acids generally considered to be weak?
by Chem_Mod
Sun Aug 21, 2011 12:08 pm
Forum: Conjugate Acids & Bases
Topic: Does Kw = [H3O+][OH-] = 1.0 x 10-14 only apply pure water?
Replies: 1
Views: 986

Re: Does Kw = [H3O+][OH-] = 1.0 x 10-14 only apply pure wat

No, it is applicable to situations in which water is the solvent. Kw is always constant for a given temperature, and that is why we can calculate pH upon addition of acid or base in the first place.
by Chem_Mod
Sun Aug 21, 2011 12:08 pm
Forum: Conjugate Acids & Bases
Topic: Does Kw = [H3O+][OH-] = 1.0 x 10-14 only apply pure water?
Replies: 1
Views: 986

Does Kw = [H3O+][OH-] = 1.0 x 10-14 only apply pure water?

Does the equation Kw = [H3O+][OH-] = 1.0 x 10-14 only apply to pure water?
by Chem_Mod
Sun Aug 21, 2011 12:07 pm
Forum: Conjugate Acids & Bases
Topic: HClO has pKa =7.53. How is it acid if its pH is >7
Replies: 1
Views: 1455

Re: HClO has pKa =7.53. How is it acid if its pH is >7

You are confused between pH and pKa which are very different. pKa tells the degree of dissociation of an acid. pKa= -logKa and Ka = [H3O+]*[A-]/[HA]. The smaller the the pKa, the larger the Ka meaning the acid is strongly dissociated into H3O+. So indeed HClO is a strong acid compare to HBrO (pKa = ...
by Chem_Mod
Sun Aug 21, 2011 12:07 pm
Forum: Conjugate Acids & Bases
Topic: HClO has pKa =7.53. How is it acid if its pH is >7
Replies: 1
Views: 1455

HClO has pKa =7.53. How is it acid if its pH is >7

HClO which has a pKa of 7.53. How is it an acid if its pH is greater than 7? Is it dependent on whether is a proton donor rather than the pH?
by Chem_Mod
Sun Aug 21, 2011 12:05 pm
Forum: Conjugate Acids & Bases
Topic: Why need autoprotolysis if the PH is greater than 6 ?
Replies: 1
Views: 366

Re: Why need autoprotolysis if the PH is greater than 6 ?

In the pH range of ~6-8, the hydronium ion concentration provided by the weak acid is comparable to that of the autoprolysis of water. Because of this, the latter cannot be ignored because neither one of the hydronium ion sources is dominant enough to ignore the other. To take into account the autop...
by Chem_Mod
Sun Aug 21, 2011 12:05 pm
Forum: Conjugate Acids & Bases
Topic: Why need autoprotolysis if the PH is greater than 6 ?
Replies: 1
Views: 366

Why need autoprotolysis if the PH is greater than 6 ?

Why must autoprotolysis need to be taken into account if the pH is greater than 6?
by Chem_Mod
Sun Aug 21, 2011 12:05 pm
Forum: Conjugate Acids & Bases
Topic: How do I know whether I am supposed to use the Ka or the Kb?
Replies: 1
Views: 11689

Re: How do I know whether I am supposed to use the Ka or the

If you have a weak base in soln then use Kb. If a weak acid then use Ka. Remember you can always convert Ka to Kb and Kb to Ka. Ka x Kb = 10^-14
by Chem_Mod
Sun Aug 21, 2011 12:04 pm
Forum: Conjugate Acids & Bases
Topic: How do I know whether I am supposed to use the Ka or the Kb?
Replies: 1
Views: 11689

How do I know whether I am supposed to use the Ka or the Kb?

How do I know whether I am supposed to use the Ka or the Kb?
by Chem_Mod
Sun Aug 21, 2011 12:04 pm
Forum: Conjugate Acids & Bases
Topic: How do you tell when to use Ka and Kb when solving problems?
Replies: 1
Views: 783

Re: How do you tell when to use Ka and Kb when solving probl

Usually Kb is used if the initial species are bases and Ka when your initial species are acids.
by Chem_Mod
Sun Aug 21, 2011 12:04 pm
Forum: Conjugate Acids & Bases
Topic: How do you tell when to use Ka and Kb when solving problems?
Replies: 1
Views: 783

How do you tell when to use Ka and Kb when solving problems?

How do you tell when to use Ka and Kb when solving problems?
by Chem_Mod
Sun Aug 21, 2011 12:03 pm
Forum: Conjugate Acids & Bases
Topic: HCO3- can act acid and base, how do you tell which it is
Replies: 1
Views: 23439

Re: HCO3- can act acid and base, how do you tell which it i

HCO3- (known as bicarbonate) is the conjugate base of H2CO3, a weak acid, and the conjugate acid of the carbonate ion. HCO3- acts as a base when mixed with a compound that is more acidic than itself (larger Ka) and as an acid when mixed with a compound that is more basic than itself (smaller Ka). Ac...
by Chem_Mod
Sun Aug 21, 2011 12:03 pm
Forum: Conjugate Acids & Bases
Topic: HCO3- can act acid and base, how do you tell which it is
Replies: 1
Views: 23439

HCO3- can act acid and base, how do you tell which it is

It seems as if HCO3- can act as both a base and an acid. How do you tell which it is?
by Chem_Mod
Sun Aug 21, 2011 12:02 pm
Forum: Conjugate Acids & Bases
Topic: KF has PH higher than 7 why KBr is neutral?
Replies: 1
Views: 782

Re: KF has PH higher than 7 why KBr is neutral?

HF is a weak acid, so F- from KF will pick up a proton from water to produce OH-.
by Chem_Mod
Sun Aug 21, 2011 12:02 pm
Forum: Conjugate Acids & Bases
Topic: KF has PH higher than 7 why KBr is neutral?
Replies: 1
Views: 782

KF has PH higher than 7 why KBr is neutral?

The pH for the KF solution is above 7, but the pH for KBr is neutral. I don't understand why they're so different.
by Chem_Mod
Sun Aug 21, 2011 12:01 pm
Forum: Conjugate Acids & Bases
Topic: How does HF, a weak acid, have F- as a weak base?
Replies: 1
Views: 927

Re: How does HF, a weak acid, have F- as a weak base?

It is a sliding scale for the strength of acids and the strength of the conjugate base. The equation Kw=Ka*Kb tells us what the books says that "the stronger the acid the weaker the conjugate base", and vice versa. However, this doesn't exclude the fact that weak acids will have weak conju...
by Chem_Mod
Sun Aug 21, 2011 12:01 pm
Forum: Conjugate Acids & Bases
Topic: How does HF, a weak acid, have F- as a weak base?
Replies: 1
Views: 927

How does HF, a weak acid, have F- as a weak base?

How does HF, a weak acid, have F- as a weak base?
by Chem_Mod
Sun Aug 21, 2011 12:01 pm
Forum: Conjugate Acids & Bases
Topic: why does KF have a pH greater than 7 and not a pH equal to 7
Replies: 1
Views: 4310

Re: why does KF have a pH greater than 7 and not a pH equal

Because F- is the anion of a weak acid (remember that HF is NOT a strong acid like the rest of the hydrohalic acids). The conjugate base of a weak acid is in fact basic in solution, raising the pH above 7. Both HBr and KOH are strong acids and bases, respectively. Conversely, Br- and K+ must be very...
by Chem_Mod
Sun Aug 21, 2011 12:00 pm
Forum: Conjugate Acids & Bases
Topic: why does KF have a pH greater than 7 and not a pH equal to 7
Replies: 1
Views: 4310

why does KF have a pH greater than 7 and not a pH equal to 7

Anions of strong acids are such weak bases that they have no significant effect on the pH of a solution and are considered basic in water, why does KF have a pH greater than 7 and not a pH equal to 7? Why is the pH 7 and not above 7 for KBr?
by Chem_Mod
Sun Aug 21, 2011 12:00 pm
Forum: Conjugate Acids & Bases
Topic: How do highly electronegative atoms diffuse net charge?
Replies: 1
Views: 335

Re: How do highly electronegative atoms diffuse net charge?

If you draw the Lewis structure for the conjugate base of HClO4 which is ClO4-. You will soon see that the anion is greatly stabilized by many resonance structures. Second, remember that O is more electronegative then Cl, so all O=Cl bonds would pull the electron densities away from the "-"...
by Chem_Mod
Sun Aug 21, 2011 11:59 am
Forum: Conjugate Acids & Bases
Topic: How do highly electronegative atoms diffuse net charge?
Replies: 1
Views: 335

How do highly electronegative atoms diffuse net charge?

How do highly electronegative atoms in a polyatomic conjugate base (like trichloroacetate) create a "chain effect" that diffuses the net charge and makes it more stable? Is this why a higher oxidation number for the central atom of an oxoacid (e.g. HClO4) makes it a stronger acid when depr...
by Chem_Mod
Sun Aug 21, 2011 11:59 am
Forum: Conjugate Acids & Bases
Topic: Strong acid-> strong or conjugate base?
Replies: 3
Views: 442

Re: Strong acid-> strong or conjugate base?

No. If you have a strong acid, that means that it is totally deprotonated in solution. A strong base would be completely protonated in solution-- so the conjugate of either would have to be weak or else, by definition, the conjugate acid or base would completely ionize again to form the original aci...
by Chem_Mod
Sun Aug 21, 2011 11:58 am
Forum: Conjugate Acids & Bases
Topic: Strong acid-> strong or conjugate base?
Replies: 3
Views: 442

Strong acid-> strong or conjugate base?

If there is a strong acid, then does that mean it has a strong or weak conjugate base? And how about for the strong base ?
by Chem_Mod
Sun Aug 21, 2011 11:57 am
Forum: Lewis Acids & Bases
Topic: Why is SbF5 considered a lewis acid?
Replies: 1
Views: 1536

Re: Why is SbF5 considered a lewis acid?

The Sb has an empty d-orbital that can accept an electron pair.
by Chem_Mod
Sun Aug 21, 2011 11:57 am
Forum: Lewis Acids & Bases
Topic: Why is SbF5 considered a lewis acid?
Replies: 1
Views: 1536

Why is SbF5 considered a lewis acid?

Why is SbF5 considered a lewis acid?
by Chem_Mod
Sun Aug 21, 2011 11:56 am
Forum: Lewis Acids & Bases
Topic: SbF5, lone pairs on F? it act as base?
Replies: 1
Views: 667

Re: SbF5, lone pairs on F? it act as base?

The Sb has an empty d-orbital while the F lone pairs are tightly held.
by Chem_Mod
Sun Aug 21, 2011 11:56 am
Forum: Lewis Acids & Bases
Topic: SbF5, lone pairs on F? it act as base?
Replies: 1
Views: 667

SbF5, lone pairs on F? it act as base?

I have a question about SbF5 as a lewis acid/base. What about all the lone pairs on the F atoms? Couldn't these be donated so that SbF(5) would act as a base? Or is it because of the electronegativity of F that that won't happen?
by Chem_Mod
Sun Aug 21, 2011 11:56 am
Forum: Lewis Acids & Bases
Topic: Compare H2O and H2S
Replies: 1
Views: 2844

Re: Compare H2O and H2S

Your reasoning is correct but there are more factors that determine e- pair availability and it turns out that H20 is more basic. Clearly their is a balance between the larger negative charge and the availability of the lone pairs. In the case of H20 versus H2S, the larger negative charge favors H20...
by Chem_Mod
Sun Aug 21, 2011 11:55 am
Forum: Lewis Acids & Bases
Topic: Compare H2O and H2S
Replies: 1
Views: 2844

Compare H2O and H2S

According to the solution manual H20 is more basic or is a stronger Lewis base than H2S because oxygen is more electronegative than S and has a higher partial negative charge. But if O is more electronegative than S, wouldn't that mean that O has a greater pulling force of electrons than S? And if t...
by Chem_Mod
Sun Aug 21, 2011 11:55 am
Forum: Lewis Acids & Bases
Topic: how to distinguish a Lewis Acid from a lewis base
Replies: 1
Views: 255

Re: how to distinguish a Lewis Acid from a lewis base

A Lewis base must have a lone pair of electrons avialable to pick up a proton. A Lewis acid must be able to accept a pair of electrons. Since boron in BF3 has 6 valence electrons it can accept 2 more giving it an octet. In many cases it is helpful to know the Lewis structure or the electron configur...
by Chem_Mod
Sun Aug 21, 2011 11:54 am
Forum: Lewis Acids & Bases
Topic: how to distinguish a Lewis Acid from a lewis base
Replies: 1
Views: 255

how to distinguish a Lewis Acid from a lewis base

I am unsure how to distinguish a Lewis Acid from a lewis base. For example, how do we know that BF3 is a Lewis acid?
by Chem_Mod
Sun Aug 21, 2011 11:54 am
Forum: Lewis Acids & Bases
Topic: Why did AlCl3 get substituted by Al(H2O)6?
Replies: 1
Views: 345

Re: Why did AlCl3 get substituted by Al(H2O)6?

Al3+ forms a complex with water as ligands and Al3+ is a Lewis acid; therefore, AlCl3 gets substituted by Al(H2O)6.
by Chem_Mod
Sun Aug 21, 2011 11:53 am
Forum: Lewis Acids & Bases
Topic: Why did AlCl3 get substituted by Al(H2O)6?
Replies: 1
Views: 345

Why did AlCl3 get substituted by Al(H2O)6?

Why did AlCl3 get substituted by Al(H2O)6?
by Chem_Mod
Sun Aug 21, 2011 11:53 am
Forum: Lewis Acids & Bases
Topic: How is AlCl3 acidic?
Replies: 1
Views: 875

Re: How is AlCl3 acidic?

Small, highly charged cations (Fe3+, Al3+, etc.,) form weekly acidic solutions by interacting with water and the water releasing a proton. When Al3+ is disolved in water, it becomes hydrated, and the hydrated form acts as a Bronsted-Lowry acid.
by Chem_Mod
Sun Aug 21, 2011 11:53 am
Forum: Lewis Acids & Bases
Topic: How is AlCl3 acidic?
Replies: 1
Views: 875

How is AlCl3 acidic?

How is AlCl3 acidic?
by Chem_Mod
Sun Aug 21, 2011 11:52 am
Forum: Lewis Acids & Bases
Topic: Why are pyridine, H+, and AlCl3 considered Lewis Acids?
Replies: 1
Views: 455

Re: Why are pyridine, H+, and AlCl3 considered Lewis Acids?

Pyridine is a base, it is basic because of the nitrogen on it that can donate its electron pair. H+ and AlCl3 are acidic because H+ and Al(3+) are electron deficient.
by Chem_Mod
Sun Aug 21, 2011 11:52 am
Forum: Lewis Acids & Bases
Topic: Why are pyridine, H+, and AlCl3 considered Lewis Acids?
Replies: 1
Views: 455

Why are pyridine, H+, and AlCl3 considered Lewis Acids?

Why are pyridine, H+, and AlCl3 considered Lewis Acids?
by Chem_Mod
Sun Aug 21, 2011 11:51 am
Forum: Lewis Acids & Bases
Topic: How to determine acidic or basic if no H+ and OH-
Replies: 1
Views: 305

Re: How to determine acidic or basic if no H+ and OH-

Electronegativity can be useful, as the more electronegative a substance is, the stronger the acid it is. Another useful tool is by considering either its lewis structure or its electron configuration and determining if it is likely to gain or lose electrons.
by Chem_Mod
Sun Aug 21, 2011 11:50 am
Forum: Lewis Acids & Bases
Topic: How to determine acidic or basic if no H+ and OH-
Replies: 1
Views: 305

How to determine acidic or basic if no H+ and OH-

How do you identify whether species are acidic or basic if presented with a molecule that doesn't have the common H- for acids and OH- for bases?
by Chem_Mod
Sun Aug 21, 2011 11:49 am
Forum: Amphoteric Compounds
Topic: Should Bi2O2 be basic or amphoteric?
Replies: 1
Views: 238

Re: Should Bi2O2 be basic or amphoteric?

It is amphoteric.
by Chem_Mod
Sun Aug 21, 2011 11:48 am
Forum: Amphoteric Compounds
Topic: Should Bi2O2 be basic or amphoteric?
Replies: 1
Views: 238

Should Bi2O2 be basic or amphoteric?

Should Bi2O2 be basic or amphoteric?
by Chem_Mod
Sun Aug 21, 2011 11:48 am
Forum: Amphoteric Compounds
Topic: In water, should we assume HSO4- acts as an acid or a base.
Replies: 1
Views: 1897

Re: In water, should we assume HSO4- acts as an acid or a ba

These compounds are amphiprotic, meaning that in water they can behave as both a proton donor or a proton acceptor (acid or a base). In general it is difficult to determine the pH of an amphiprotic compound (how to do that is discussed more in Section 10.15, which is not part of your assigned readin...
by Chem_Mod
Sun Aug 21, 2011 11:48 am
Forum: Amphoteric Compounds
Topic: In water, should we assume HSO4- acts as an acid or a base.
Replies: 1
Views: 1897

In water, should we assume HSO4- acts as an acid or a base.

In water, should we assume HSO4- acts as an acid or a base. Also for HCO3-?
by Chem_Mod
Sun Aug 21, 2011 11:48 am
Forum: Amphoteric Compounds
Topic: Why is the formula pH=(1/2)(pKa1+pKa2) used?
Replies: 1
Views: 7508

Re: Why is the formula pH=(1/2)(pKa1+pKa2) used?

The formula is used when a polyprotic compound is amphiprotic (it acts as both an acid and a base). Because it can behave as both, it is not obvious if the pH will be acidic or basic. Noting that a high pKa means a small Ka value, having both high pKa1 and pKa2 values tells you that the polyprotic c...
by Chem_Mod
Sun Aug 21, 2011 11:47 am
Forum: Amphoteric Compounds
Topic: Why is the formula pH=(1/2)(pKa1+pKa2) used?
Replies: 1
Views: 7508

Why is the formula pH=(1/2)(pKa1+pKa2) used?

Why is the formula pH=(1/2)(pKa1+pKa2) used?
by Chem_Mod
Sun Aug 21, 2011 11:47 am
Forum: Amphoteric Compounds
Topic: NH3 (aq) + H2O (l) --> NH4+(aq) + OH- (aq), acid and base?
Replies: 1
Views: 23878

Re: NH3 (aq) + H2O (l) --> NH4+(aq) + OH- (aq), acid and bas

Yes. Remember water can act as an acid or a base. In this case, water gives off proton, water is an acid.
by Chem_Mod
Sun Aug 21, 2011 11:46 am
Forum: Amphoteric Compounds
Topic: NH3 (aq) + H2O (l) --> NH4+(aq) + OH- (aq), acid and base?
Replies: 1
Views: 23878

NH3 (aq) + H2O (l) --> NH4+(aq) + OH- (aq), acid and base?

In the reaction NH3 (aq) + H2O (l) --> NH4+(aq) + OH- (aq), NH3 is the weak base, but does that mean that H2O is considered an acid because it donates its proton to form OH-?
by Chem_Mod
Sun Aug 21, 2011 11:46 am
Forum: Amphoteric Compounds
Topic: particular d-block metals form amphoteric oxides?
Replies: 1
Views: 2161

Re: particular d-block metals form amphoteric oxides?

We covered metal oxides and hydroxides (e.g., NaOH) which are basic compounds. We also covered non-metal oxides (e.g., H2SO4, H3PO4, etc.,) which are acidic compounds. The metalloids (diagonal band between metals and nonmetals) form amphoteric compounds, that is they can act like an acid or base. So...
by Chem_Mod
Sun Aug 21, 2011 11:46 am
Forum: Amphoteric Compounds
Topic: particular d-block metals form amphoteric oxides?
Replies: 1
Views: 2161

particular d-block metals form amphoteric oxides?

The book mentions that d-block metals form acidic, amphoteric, or basic oxides form depending on their oxidation state. Are they saying that particular d-block metals form amphoteric oxides, and if so, which ones?
by Chem_Mod
Sun Aug 21, 2011 11:45 am
Forum: Amphoteric Compounds
Topic: How to determine oxides are acidic, basic, or amphoteric
Replies: 1
Views: 4264

Re: How to determine oxides are acidic, basic, or amphoteric

In general, metal oxides (i.e. CaO) are basic while nonmetal oxides (i.e. CO2) are acidic. Oxides made with the elements known as metalloids (B, Si, Ge, As, Sb, Te, and Po) can be acidic or basic depending on their environment; in other words they are amphoteric. (However, this general trend cannot ...
by Chem_Mod
Sun Aug 21, 2011 11:45 am
Forum: Amphoteric Compounds
Topic: How to determine oxides are acidic, basic, or amphoteric
Replies: 1
Views: 4264

How to determine oxides are acidic, basic, or amphoteric

How do we determine whether oxides are acidic, basic, or amphoteric?
by Chem_Mod
Sun Aug 21, 2011 11:44 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Are noble gases considered bases?
Replies: 3
Views: 790

Re: Are noble gases considered bases?

No. Noble gases are mostly unreactive and do not act as bases.
by Chem_Mod
Sun Aug 21, 2011 11:44 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Are noble gases considered bases?
Replies: 3
Views: 790

Are noble gases considered bases?

Are noble gases considered bases?
by Chem_Mod
Sun Aug 21, 2011 11:43 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why is [Ba(OH)2]=[Ba2+]?
Replies: 1
Views: 582

Re: Why is [Ba(OH)2]=[Ba2+]?

Because it is a 1:1 molar ratio. 1 mole of Ba(OH)2 gives 1 mole of Ba2+.
by Chem_Mod
Sun Aug 21, 2011 11:43 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why is [Ba(OH)2]=[Ba2+]?
Replies: 1
Views: 582

Why is [Ba(OH)2]=[Ba2+]?

Why is [Ba(OH)2]=[Ba2+]?
by Chem_Mod
Sun Aug 21, 2011 11:43 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: dissociation of Ba(OH)2, why multiply OH by 2
Replies: 1
Views: 5370

Re: dissociation of Ba(OH)2, why multiply OH by 2

When one molecule of Ba(OH)2 dissolves in water, it dissociates to (Ba2+) + (2 x OH-). You are not writing the equilibrium constant, so you should not raise it to the power of 2.
by Chem_Mod
Sun Aug 21, 2011 11:43 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: dissociation of Ba(OH)2, why multiply OH by 2
Replies: 1
Views: 5370

dissociation of Ba(OH)2, why multiply OH by 2

For the dissociation of Ba(OH)2, why it is necessary to multiply [OH-] by 2, instead of raising it to the power of 2?
by Chem_Mod
Sun Aug 21, 2011 11:42 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Can conjugate acids of strong bases be neutral?
Replies: 1
Views: 355

Re: Can conjugate acids of strong bases be neutral?

All of the strong bases are hydroxides which, upon complete dissociation, form the hydroxide ion and an ionic salt. The ionic salt has no effect on the pH; therefore, the salt of a strong base is neutral. Note that these salts are not Bronsted acids because they are aprotic (no protons to give).
by Chem_Mod
Sun Aug 21, 2011 11:42 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Can conjugate acids of strong bases be neutral?
Replies: 1
Views: 355

Can conjugate acids of strong bases be neutral?

Can conjugate acids of strong bases be neutral?
by Chem_Mod
Sun Aug 21, 2011 11:41 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why CaO and Na2O act as strong base when dissolved in water
Replies: 1
Views: 1498

Re: Why CaO and Na2O act as strong base when dissolved in w

It is because these two species readily form Ca(OH)2 and NaOH in water.
by Chem_Mod
Sun Aug 21, 2011 11:41 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why CaO and Na2O act as strong base when dissolved in water
Replies: 1
Views: 1498

Why CaO and Na2O act as strong base when dissolved in water

Why do CaO and Na2O act as strong bases when dissolved in water while the others do not?
by Chem_Mod
Sun Aug 21, 2011 11:40 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why are Group 1 or Group 2 oxides strong bases?
Replies: 1
Views: 822

Re: Why are Group 1 or Group 2 oxides strong bases?

A group 1 or group 2 oxide is a strong base because when added to water, it produces OH-. An example of a basic Group 1 oxide is Na2O and an example of a basic Group 2 oxide is CaO.
by Chem_Mod
Sun Aug 21, 2011 11:40 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: Why are Group 1 or Group 2 oxides strong bases?
Replies: 1
Views: 822

Why are Group 1 or Group 2 oxides strong bases?

Why are Group 1 or Group 2 oxides strong bases? What are some examples of these types of strong bases?
by Chem_Mod
Sun Aug 21, 2011 11:40 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: How do we find the concentration of a strong base?
Replies: 1
Views: 285

Re: How do we find the concentration of a strong base?

For strong bases the concentration of OH- will be the same as the concentration of the base itself. For example, the concentration of NaOH = concentration of OH-.
by Chem_Mod
Sun Aug 21, 2011 11:40 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: How do we find the concentration of a strong base?
Replies: 1
Views: 285

How do we find the concentration of a strong base?

How do we find the concentration of a strong base?
by Chem_Mod
Sun Aug 21, 2011 11:39 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: How can we differentiate some molecules as acids or bases?
Replies: 1
Views: 319

Re: How can we differentiate some molecules as acids or base

Compare it to a familiar molecule. In this case, NH3, which acts as a base, so the molecule NH2NH2 is likely to be basic.
by Chem_Mod
Sun Aug 21, 2011 11:39 am
Forum: Properties & Structures of Inorganic & Organic Bases
Topic: How can we differentiate some molecules as acids or bases?
Replies: 1
Views: 319

How can we differentiate some molecules as acids or bases?

How can we differentiate some molecules as acids or bases. For example, how do we know that NH2NH2 is a base and not an acid?
by Chem_Mod
Sun Aug 21, 2011 11:38 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Why is HCl a weaker acid than HBr and HI?
Replies: 1
Views: 6921

Re: Why is HCl a weaker acid than HBr and HI?

HCl has a short (stronger) bond than HBr and HI. Thus HBr and HI give up their protons more readily due to the longer bond length and are stronger acids. For Hypobromous and hypoiodous acid, the electronegative bromine and iodine slightly reduce the electronegativity of the oxygen atom
by Chem_Mod
Sun Aug 21, 2011 11:38 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Why is HCl a weaker acid than HBr and HI?
Replies: 1
Views: 6921

Why is HCl a weaker acid than HBr and HI?

Why is HCl a weaker acid than HBr and HI if it has a greater electronegativity, but then stronger than Hypobromous Acid and Hypoiodous Acid?

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