I was able to answer Regions 1 and 2.But I really need help with region 3! and p

Question

I was able to answer Regions 1 and 2.But I really need help with region 3! and please show all work and tables!Thank you!

For all of the following questions 10.00 mL of 0.187 M acetic acid (CH3COOH) is titrated with 0.100 M KOH (The Ka of acetic acid is 1.80 x 10) Region 1: Initial pH Before any titrant is added to the starting material 1. Which of the following statements are true about BCA tables and ICE tables? (Choose all that apply) A balanced chemical equation is needed to use an ICE table and BCA table An ICE table requires units of moles while a BCA table requires units of concentration An ICE table requires units of concentration while a BCA table requires units of moles O ICE tables and BCA tables can be used interchangeably. 2. Complete the ICE table below at this point in the titration. Be sure your Change and Equilibrium lines include the variable "X". Do not calculate "x" for this question CH3COOH(aq)H+(aq) CH3COO(aq) Initial concentration (M)0.187 Change in concentration (M) +X +X Equilibrium concentration (M) 0.187-x 3. Use the Ka expression and determine the concentration of H and the pH of this solution x 10-3 - [H+]: 1.83 M pH2.74

Explanation / Answer

Region 3

Q8. At the equivalence point, we know that no. of moles of acid = no. of moles of base. So, we use the formula,

MaVa = MbVb

Ma = molarity of acid = 0.187M

Va = volume of acid = 10mL

Mb = Molarity of base = 0.1M

Vb = volume of base?

So, 0.187M x 10mL = 0.1M x Vb

Vb = 18.7mL

Volume of titrant added at equivalence point = 18.7mL

(One question at a time.)

Have a nice day!

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