Search found 60 matches

by Shail Avasthi 3C
Sun Jan 19, 2020 5:35 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: ICE table
Replies: 11
Views: 32

Re: ICE table

An ICE table should be used when you are given initial concentrations and are asked to find concentrations, pH, or pOH at equilibrium. You should memorize the strong acids and strong bases.
by Shail Avasthi 3C
Sun Jan 19, 2020 5:33 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: pH vs. pOH
Replies: 13
Views: 27

Re: pH vs. pOH

You calculate pH and pOH by taking the negative log (-log) of [H3O+] or [OH-]. You typically calculate pH for acids and pOH for bases, but questions will often ask you for pH no matter what. Use pH+pOH=14 to convert from pOH to pH.
by Shail Avasthi 3C
Sun Jan 19, 2020 5:31 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: conjugate seesaw
Replies: 4
Views: 13

Re: conjugate seesaw

Ka x Kb = Kw
Kw is a constant (10^-14)
If Ka is high for a strong acid, Kb must therefore be low because their product is equal to a constant. And vice versa: if Kb is high for a strong base, then Ka must therefore be low.
by Shail Avasthi 3C
Sun Jan 19, 2020 5:28 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: % Ionization
Replies: 3
Views: 9

Re: % Ionization

@AMahadi, if your Ka or Kb is small (<10^-3), then you are allowed to eliminate all x values in the equilibrium expression which follows the form (n-x). This makes calculating the value of x more simple. If the percent ionization of the acid or base is <5%, then this approximation is valid.
by Shail Avasthi 3C
Sun Jan 19, 2020 5:24 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: kA and kB
Replies: 1
Views: 5

Re: kA and kB

Ka x Kb = Kw (10^-14)
pKa + pKb = 14
by Shail Avasthi 3C
Sat Jan 11, 2020 8:58 pm
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Using the "ICE" box
Replies: 8
Views: 55

Re: Using the "ICE" box

Don't include solids and liquids in equilibrium calculations.
by Shail Avasthi 3C
Sat Jan 11, 2020 8:54 pm
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Using Kc Vs Kp
Replies: 7
Views: 31

Re: Using Kc Vs Kp

If you're looking at aqueous equilibrium, use Kc. If looking at gasses, you can either use Kc or Kp. Use the question to determine the proper answer.
by Shail Avasthi 3C
Sat Jan 11, 2020 8:52 pm
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Problem 5i.11- using molarity in place of pressure?
Replies: 3
Views: 24

Re: Problem 5i.11- using molarity in place of pressure?

You can either use partial pressure or concentration when calculating equilibrium for gasses.
by Shail Avasthi 3C
Sat Jan 11, 2020 8:51 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: 5.35
Replies: 4
Views: 37

Re: 5.35

Create an ICE table using the initial and final values for A B and C in the table. Then plug these values into the K expression.
by Shail Avasthi 3C
Sat Jan 11, 2020 8:45 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Difference between K and Q
Replies: 6
Views: 22

Re: Difference between K and Q

K is the ratio of the concentrations of the products and reactants when the reaction is at equilibrium. Q is the ratio of the concentrations of the products and reactants at any point in the reaction. Comparing K to Q will tell you which way the reaction will proceed.
by Shail Avasthi 3C
Tue Dec 03, 2019 8:13 pm
Forum: Electronegativity
Topic: Symbols for partial charge
Replies: 4
Views: 35

Re: Symbols for partial charge

The +/- delta symbols represent partial positive and partial negative. The +-----> arrow points in the direction of the negative end of the dipole, with the "cross" end of the arrow towards the positive end of the dipole.
by Shail Avasthi 3C
Tue Dec 03, 2019 8:09 pm
Forum: Amphoteric Compounds
Topic: how to determine
Replies: 3
Views: 24

Re: how to determine

No. Take the amphoteric oxides as an example (e.g. Al2O3). If you react Al2O3 with a strong acid, it will act as a base by producing hydroxide ions. If you react Al2O3 with a strong base, it will act as an acid by producing hydronium ions. None of the amphoteric oxides contain hydrogen.
by Shail Avasthi 3C
Tue Dec 03, 2019 7:59 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Explain VSEPR conceptually
Replies: 12
Views: 51

Re: Explain VSEPR conceptually

VSEPR predicts the shapes of molecules by using the principle that regions of electron density around a central atom will tend to maximize their distance from one another. This principle leads to the various VSEPR geometries, such as trigonal bipyramidal, tetrahedral, etc. These shapes maximize the ...
by Shail Avasthi 3C
Tue Dec 03, 2019 7:57 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: Bent vs linear
Replies: 56
Views: 284

Re: Bent vs linear

Bent molecules will have lone pairs on the central atom in addition to the two bound atoms. These lone pairs will distort the shape of the molecule to bent instead of linear.
by Shail Avasthi 3C
Tue Dec 03, 2019 7:56 pm
Forum: Determining Molecular Shape (VSEPR)
Topic: T-shape
Replies: 21
Views: 96

Re: T-shape

T shaped molecules have 3 bonded atoms and 2 lone pairs. The 5 regions of electron density have trigonal bipyramidal geometry, and the two lone pairs are placed equatorially to maximize distance; this forms a T shaped molecule.
by Shail Avasthi 3C
Tue Dec 03, 2019 7:53 pm
Forum: Calculating the pH of Salt Solutions
Topic: pKa vs Ka
Replies: 6
Views: 39

Re: pKa vs Ka

For the following acid equilibrium :

HA <----> H+ + A-

Ka = [H+][A-]/[HA]

pKa = -log[Ka]
by Shail Avasthi 3C
Tue Dec 03, 2019 7:50 pm
Forum: Polyprotic Acids & Bases
Topic: How can you tell
Replies: 11
Views: 91

Re: How can you tell

If an acid has more than one hydrogen which it can dissociate, it is polyprotic.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:34 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Pka vs Ka
Replies: 10
Views: 76

Re: Pka vs Ka

For the following reaction:

HA ---> H+ + A-

Ka = [H+][A-]/[HA]
pKa = -log(Ka)

For stronger acids, Ka will be high and pKa will be low, and vice versa.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:32 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Inorganic or Organic
Replies: 6
Views: 31

Re: Inorganic or Organic

Organic = Carbon. Therefore, organic acids have carbon while inorganic acids do not.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:31 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Difference between weak acids/bases and strong acids/bases
Replies: 6
Views: 34

Re: Difference between weak acids/bases and strong acids/bases

Strong acids fully ionize (i.e. dissociate into products), while weak acids only partially dissociate and require equilibrium calculations to determine concentrations etc.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:30 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Strong Acids
Replies: 3
Views: 29

Re: Strong Acids

The Ka is equal to the product of the concentrations of the products divided by the product of the concentrations of the reactants. e.g.: HA ---> H+ + A- Ka = [H+][A-]/[HA] Stronger acids more readily dissociate into their products. Therefore, the stronger the acid, the higher the Ka because the con...
by Shail Avasthi 3C
Mon Dec 02, 2019 10:25 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Acids Vs. Bases
Replies: 11
Views: 55

Re: Acids Vs. Bases

Acids typically lose H+ while bases typically gain them.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:23 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Strength of Acids - Example from Lecture
Replies: 6
Views: 34

Re: Strength of Acids - Example from Lecture

CCl3COOH and CH3COOH have the anions CCl3COO- and CH3COO- respectively. The former anion is more stable than the latter because the 3 chlorines delocalize the negative charge on the oxygen. Oxoacids will be more acidic if the resulting anion is stabilized by electronegative atoms which delocalize th...
by Shail Avasthi 3C
Mon Dec 02, 2019 10:19 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Trichloroacetic acid
Replies: 2
Views: 21

Re: Trichloroacetic acid

The resulting anion of trichloroacetic acid is more stable than that of acetic acid because the three chlorines delocalize the negative charge on the oxygen, whereas in acetic acid, the charge is not as delocalized. Oxoacids which have more stable anions will be more acidic.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:15 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Amphoteric compounds
Replies: 4
Views: 28

Re: Amphoteric compounds

Amphoteric compounds can have both acidic and basic character. (e.g. H2O can become H3O+ or OH-)

Dr. Lavelle pointed out in class the diagonal band of amphoteric oxides (Be, Al, Ga, Sn, Sb, Pb), quite similar to the band of metalloids. All of these oxides (e.g. Al2O3) are amphoteric.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:11 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: neutralization
Replies: 4
Views: 22

Re: neutralization

Neutralization reactions form water and a salt as their products.
by Shail Avasthi 3C
Mon Dec 02, 2019 10:08 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Lecture
Replies: 3
Views: 32

Re: Lecture

Compare the acids HClO and HBrO. Their resulting anions will be ClO- and BrO- respectively. ClO- will be more stable than BrO for the following reason: Chlorine and Bromine are both considered "electron-withdrawing atoms" because of their electronegativity, and they will have the effect of...
by Shail Avasthi 3C
Mon Dec 02, 2019 10:03 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Electronegativity and acid strength
Replies: 5
Views: 28

Re: Electronegativity and acid strength

Oxoacids will be more acidic if the anion formed is stabilized by electronegative atoms which delocalize the negative charge. Chlorine is more electronegative than bromine, which means it will more effectively delocalize the negative charge on the oxygen, yielding a more stable anion – this causes i...
by Shail Avasthi 3C
Mon Dec 02, 2019 10:03 am
Forum: Properties & Structures of Inorganic & Organic Acids
Topic: Electronegativity and acid strength
Replies: 2
Views: 12

Re: Electronegativity and acid strength

Oxoacids will be more acidic if the anion formed is stabilized by electronegative atoms which delocalize the negative charge. Chlorine is more electronegative than bromine, which means it will more effectively delocalize the negative charge on the oxygen, yielding a more stable anion – this causes i...
by Shail Avasthi 3C
Fri Nov 15, 2019 1:09 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Remembering Molecular Geometric Shapes
Replies: 2
Views: 18

Re: Remembering Molecular Geometric Shapes

https://lh6.googleusercontent.com/fH1A2_-wM47qFR8X69w6002x-Iw75lx2Lxh6WiY4oTErTr2YyOOluabl5HuJ0usijqiz1QxAQSuuXIDl67mF1AwouYEiNtxQgShsJWJkDqEhFOoSuTIM5ORfbP9O You could memorize, the 5 "parent" shapes (linear, trigonal pyramidal, tetrahedral, trigonal bipyramidal, octahedral), and then in...
by Shail Avasthi 3C
Fri Nov 15, 2019 1:04 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Determining Bond Angle
Replies: 3
Views: 21

Re: Determining Bond Angle

Not always. For example, in square planar molecules, the bond angles are still 90 degrees because the axial lone pairs directly oppose each other. Another example would be linear molecules with three equatorial lone pairs: the bond angle is still 180 degrees.
by Shail Avasthi 3C
Fri Nov 15, 2019 1:00 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Molecular Geometry vs Electron Geometry
Replies: 2
Views: 22

Re: Molecular Geometry vs Electron Geometry

The electron geometry is the arrangement of the regions of electron density (lone pairs + bonding regions) around the central atom. The molecular geometry is the shape of the molecule, which is only determined using the bonding regions. For example, the electron geometry of H2O is tetrahedral becaus...
by Shail Avasthi 3C
Fri Nov 15, 2019 12:55 am
Forum: Determining Molecular Shape (VSEPR)
Topic: bond angles
Replies: 9
Views: 40

Re: bond angles

Lone pairs have greater repulsion strength than bonding regions do. So lone pairs will tend to push bonding regions closer together, making the bond angles "a little less then" their typical value. For example, if you have a tetrahedral with 1 lone pair, the three bonding regions will have...
by Shail Avasthi 3C
Fri Nov 15, 2019 12:54 am
Forum: Determining Molecular Shape (VSEPR)
Topic: Octahedral
Replies: 5
Views: 24

Re: Octahedral

All three have the 6 regions of electron density arranged as an octahedral. The difference is in the number of lone pairs and the number of bonding regions. If the molecular shape is an octahedral, then it has 6 bonding regions (i.e. 6 atoms bound to the central atom). If the molecular shape is squa...
by Shail Avasthi 3C
Fri Nov 15, 2019 12:48 am
Forum: Hybridization
Topic: Pi and Sigma Bonds
Replies: 17
Views: 320

Re: Pi and Sigma Bonds

Every bond after the first is a pi bond. (i.e. single bond = 1 sigma ; double bond = 1 sigma & 1 pi ; triple bond = 1 sigma & 2 pi)
by Shail Avasthi 3C
Mon Nov 11, 2019 11:17 pm
Forum: Lewis Structures
Topic: Drawing Lewis Structures
Replies: 18
Views: 71

Re: Drawing Lewis Structures

As others have said, formal charges must add up to the overall charge of the molecule you are drawing. However, when it comes to determining which atom(s) gets the non-zero formal charge(s), use electronegativity. For example, if you draw the lewis structure for the chlorate ion (ClO3-), when decidi...
by Shail Avasthi 3C
Mon Nov 11, 2019 11:12 pm
Forum: Lewis Structures
Topic: Lewis structures that are not symmetrical
Replies: 4
Views: 32

Re: Lewis structures that are not symmetrical

It depends on the molecule. When you arrange 5 identical atoms around a central atom (e.g. PF5), this molecule will be non-polar because of the shape of the molecule. You can also have a symmetrical molecule that is polar (e.g. CH2Cl2) due to dipole moments etc.. Symmetry is not a reliable way to de...
by Shail Avasthi 3C
Mon Nov 11, 2019 11:02 pm
Forum: Lewis Structures
Topic: Center of a Lewis Structure
Replies: 7
Views: 40

Re: Center of a Lewis Structure

Yes. Lavelle said in lecture that this is the best way of going about drawing lewis structures for this class.
by Shail Avasthi 3C
Mon Nov 11, 2019 10:56 pm
Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
Topic: melting points
Replies: 6
Views: 37

Re: melting points

Hydrogen bonds are stronger than dipole/dipole or induced dipole/induced dipole interactions. H2O has the ability to hydrogen bond with itself because of the H-O bond, while H2S cannot. This accounts for H2O's higher melting point.
by Shail Avasthi 3C
Mon Nov 11, 2019 10:53 pm
Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
Topic: Homework 3F.5 Part C
Replies: 2
Views: 29

Re: Homework 3F.5 Part C

CHI3 is a much larger molecule than CHF3, because the size of Iodine's electron cloud is much larger than the size of Fluorine's. The larger the molecule (by molar mass and by size), the greater its polarizability and therefore the greater its LDFs (induced dipole/induced dipole)
by Shail Avasthi 3C
Sun Nov 03, 2019 11:50 pm
Forum: Polarisability of Anions, The Polarizing Power of Cations
Topic: Differences between polarizing power and polarizablity
Replies: 2
Views: 31

Re: Differences between polarizing power and polarizablity

Cations have polarizing power because their positive charge distorts the electron cloud of the anion. Likewise, anions have polarizability because their electron cloud can be distorted by positively charged cations. The greater the charge on the cation (Al3+ is a good example), the higher its polari...
by Shail Avasthi 3C
Sun Nov 03, 2019 11:46 pm
Forum: Lewis Structures
Topic: Drawing lewis structures
Replies: 5
Views: 37

Re: Drawing lewis structures

Try and minimize your formal charges whenever you draw a Lewis structure, because this means that you have likely found the most stable structure.
by Shail Avasthi 3C
Sun Nov 03, 2019 11:44 pm
Forum: Lewis Structures
Topic: formal charge
Replies: 6
Views: 27

Re: formal charge

Formal charges are a useful quick check to see if your Lewis Structure is stable or still needs reworking. I would recommend quickly checking formal charges on most lewis structures you draw for this reason, unless it's ridiculously easy or it's a structure you know already.
by Shail Avasthi 3C
Sun Nov 03, 2019 8:30 pm
Forum: DeBroglie Equation
Topic: Dino Nuggets Problem 6a
Replies: 2
Views: 70

Re: Dino Nuggets Problem 6a

Actually I figured it out, but I'm going to keep this here in case anyone else is confused. The power of 10 is off by 3 because I forgot to convert grams to kilograms...
by Shail Avasthi 3C
Sun Nov 03, 2019 8:27 pm
Forum: DeBroglie Equation
Topic: Dino Nuggets Problem 6a
Replies: 2
Views: 70

Dino Nuggets Problem 6a

(Problem: A new element GarBreadium is discovered to have molar mass 3.157 g∙mol-1. The GarBreadium atom travels at an average speed of 1.35x103 m∙s-1 at room temperature. What is the average wavelength of the GarBreadium atom at room temperature?) My answer for this problem comes out to 9.36x10^-14...
by Shail Avasthi 3C
Sun Oct 27, 2019 10:27 pm
Forum: Lewis Structures
Topic: Choosing the central atom
Replies: 16
Views: 69

Re: Choosing the central atom

The atom with the lowest ionization energy should be the central atom. When a molecule contains carbon, it is usually central in some way. Hydrogen should never be chosen as the central atom.
by Shail Avasthi 3C
Sun Oct 27, 2019 10:23 pm
Forum: Formal Charge and Oxidation Numbers
Topic: Formal charge purpose
Replies: 40
Views: 1676

Re: Formal charge purpose

Formal charges also allow you to compare different possible lewis structures for the same molecule. For example, if the oxygen atoms in one lewis structure have positive formal charges and negative formal charges in another, the second lewis structure is probably preferable (assuming that other fact...
by Shail Avasthi 3C
Sun Oct 27, 2019 10:20 pm
Forum: Sigma & Pi Bonds
Topic: Double bond
Replies: 15
Views: 107

Re: Double bond

Add double bonds to a lewis structure when you still need to satisfy the octet rule after adding your valence electrons, or if it gives the molecule better formal charges.
by Shail Avasthi 3C
Sun Oct 27, 2019 10:17 pm
Forum: Lewis Structures
Topic: Choosing the central atom
Replies: 16
Views: 69

Re: Choosing the central atom

The atom with the lowest ionization energy should be the central atom.
by Shail Avasthi 3C
Sun Oct 27, 2019 10:14 pm
Forum: Ionic & Covalent Bonds
Topic: What is the difference between an anion and cation?
Replies: 7
Views: 41

Re: What is the difference between an anion and cation?

An anion is an ion with a negative charge and a cation is an ion with a positive charge. (The way I remember this is that the "t" in cation looks like a plus sign which makes it positively charged.)
by Shail Avasthi 3C
Sun Oct 20, 2019 9:10 pm
Forum: Electron Configurations for Multi-Electron Atoms
Topic: magnetic quantum #
Replies: 3
Views: 31

Re: magnetic quantum #

Different subscripts for different orbitals (e.g. px, py, pz, dxy, dyz, dxy, etc.) are just different labels for the possible orientations of the orbitals of a certain shape, based on the coordinate system you are using. In other words, for ml = -1, 0, 1, it is arbitrary which one you label as px, p...
by Shail Avasthi 3C
Sun Oct 20, 2019 9:02 pm
Forum: Electron Configurations for Multi-Electron Atoms
Topic: Pauli Exclusion Principle
Replies: 9
Views: 53

Re: Pauli Exclusion Principle

No two electrons may have the same 4 quantum numbers. i.e. two electrons in the same orbital must have opposite spins. It is not possible for them to have the same spin.
by Shail Avasthi 3C
Sun Oct 20, 2019 8:59 pm
Forum: Trends in The Periodic Table
Topic: Trends in Electron Affinity
Replies: 3
Views: 49

Re: Trends in Electron Affinity

Electron affinity tends to increase as atoms get more electronegative, i.e. moving up and to the right on the periodic table.
by Shail Avasthi 3C
Sun Oct 20, 2019 8:54 pm
Forum: Trends in The Periodic Table
Topic: Atomic Radius
Replies: 16
Views: 145

Re: Atomic Radius

You should only compare atomic radii of atoms in their ground state.
by Shail Avasthi 3C
Sun Oct 20, 2019 8:52 pm
Forum: Trends in The Periodic Table
Topic: Atomic radii
Replies: 9
Views: 47

Re: Atomic radii

As you move right across a row in the periodic table, the positive charge of the nucleus becomes greater due to the increasing number of protons. This causes the nucleus to have a greater pull on the electrons, thereby decreasing the atomic radius. This is the effect of effective nuclear charge.
by Shail Avasthi 3C
Sat Oct 12, 2019 5:21 pm
Forum: Empirical & Molecular Formulas
Topic: post test problem
Replies: 3
Views: 91

Re: post test problem

Yes, understanding conservation of mass is key to solving this problem. The amount of Cobalt is unchanged in the reactants and products, so to find the mass of Fluorine used, you need to subtract the mass of Cobalt (339.20 g) from the final mass of the products (996.08), which you can use to solve t...
by Shail Avasthi 3C
Sat Oct 12, 2019 5:17 pm
Forum: Significant Figures
Topic: Question About Significant Figures and Rounding
Replies: 22
Views: 303

Re: Question About Significant Figures and Rounding

Don't worry about significant figures until it's time to write your final answer to the problem. While solving the problem, numbers should remain as exact as possible so that your final answer is as accurate as it can be. Then apply significant figure rules to your final answer.
by Shail Avasthi 3C
Sat Oct 12, 2019 5:14 pm
Forum: Significant Figures
Topic: Answer being a tad bit off
Replies: 8
Views: 143

Re: Answer being a tad bit off

Try to avoid rounding the numbers you use for your calculation, and only round at the end of the problem. Excess rounding while solving a problem leads to significant discrepancies between your answer and the correct answer.
by Shail Avasthi 3C
Sat Oct 12, 2019 5:11 pm
Forum: Limiting Reactant Calculations
Topic: Test 1 Calculator
Replies: 6
Views: 107

Re: Test 1 Calculator

In addition, many new graphing calculators have systems of equations solvers which significantly cuts down the time required to solve certain problems later on in the course.
by Shail Avasthi 3C
Sat Oct 12, 2019 4:57 pm
Forum: Molarity, Solutions, Dilutions
Topic: L37
Replies: 3
Views: 74

Re: L37

a) Typically for dilution problems you want to look for a way to use M1V1 = M2V2 if possible. In this case we are given 3 knowns (concentrated molarity, final molarity, and final volume) and one unknown (concentrated volume). When we plug these into M1V1 = M2V2, we get the following: (16 M concentra...

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