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AP CHEM question! Can you please follow these steps for each: 1.) net ionic equation, 2.)...

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Chemistry

AP CHEM question! Can you please follow these steps foreach: 1.) net ionic equation, 2.) ice table, 3.) pH= pKa + log(CB/WA)

A 35.0 mL sample of 0.150 M acetic acid (HC2H3O2) is titratedwith 0.150 M NaOH solution. Calculate the pH after the followingvolumes of base have been added:

A.) 0 mL
B.) 17.5 mL
C.) 34.5 mL
D.) 35.0 mL
E.) 35.5 mL
F.) 50.0 mL

Answer & Explanation Solved by verified expert
4.3 Ratings (826 Votes)
1when 00 mL of NaOH is added HC2H3O2 dissociates as HC2H3O2 H C2H3O2 015 0 0 015x x x Ka HC2H3O2HC2H3O2 Ka xxcx Assuming x can be ignored as compared to c So above expression becomes Ka xxc so x sqrt Kac x sqrt 175105015 162103 since x is comparable c our assumption is not correct we need to solve this using Quadratic equation Ka xxcx 175105 x2015x 2625106 175105 x x2 x2 175105 x2625106 0 This is quadratic equation ax2bxc0 a 1 b 175105 c 2625106 Roots can be found by x b sqrtb24ac2a x b sqrtb24ac2a b24ac 105105 roots are x 1611103 and x 1629103 since x cant be negative the possible value of x is x 1611103 use pH log H log 1611103 27928 2when 175 mL of NaOH is added Given    See Answer
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