question 6B.7

Moderators: Chem_Mod, Chem_Admin

Jade Hinds 2B
Posts: 75
Joined: Tue Sep 10, 2019 12:16 am

question 6B.7

Postby Jade Hinds 2B » Sun Jan 19, 2020 6:30 pm

The pH of several solutions was measured in research laboratories of a food company; convert each of the following pH values into the molar concentration of H3O+ ions: (a) 3.3 (the pH of sour orange juice); (b) 6.7 (the pH of the saliva sample); (c) 4.4 (the pH of beer); (d) 5.3 (the pH of a coffee sample)

Tanmay Singhal 1H
Posts: 143
Joined: Sat Jul 20, 2019 12:16 am

Re: question 6B.7

Postby Tanmay Singhal 1H » Sun Jan 19, 2020 6:35 pm

i believe it is 10^(of the ph)

Baoying Li 1B
Posts: 113
Joined: Sat Aug 17, 2019 12:18 am

Re: question 6B.7

Postby Baoying Li 1B » Sun Jan 19, 2020 6:58 pm

Since pH=-log[H3O+}, the concentration of H3O+ would be 10 to the -pH.

Rodrigo2J
Posts: 102
Joined: Sat Jul 20, 2019 12:16 am

Re: question 6B.7

Postby Rodrigo2J » Sun Jan 19, 2020 7:00 pm

To convert from pH to [H3O+] you just need to use the equation [H3O+]= 10^(-pH).

Bryce Ramirez 1J
Posts: 120
Joined: Sat Aug 24, 2019 12:16 am

Re: question 6B.7

Postby Bryce Ramirez 1J » Sun Jan 19, 2020 9:13 pm

Make sure to remember that significant figures for logs involves the numbers after the decimal. So if there were two significant figures given in the problem, setting up the equation for pH would involve using two significant figures after the decimal point.


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests