Calculate the pH of a 1.00 L solution that is 0.100 M HC_2H_3O_2 and 0.100 M NaC

Question

Calculate the pH of a 1.00 L solution that is 0.100 M HC_2H_3O_2 and 0.100 M NaC_2H_3O_2. PH = The solution in Q3 is called a buffer solution. The important charateristic of a buffer solution is its ability to resist large changes in pH when small amounts of strong acid or strong base are added. Consider the pH calculated in Q3, if a small amount of HCI is added to the solution will the pH increase or decrease? Provide a short response explaining y our answer. In 1.00 Liter of solution that is 0.100 M HC_2H_3O_2 and 0.100 M NaC_2H_3O_2 what is the formula of the weak acid and the formula of the weak base in the solution weak acid component of the buffer weak base component of the buffer If some HCI is added to the buffer solution in Q5 write a chemical equation that describes how the buffer solution neutralizes the added HCI. If some NaOH is added to the buffer solution in Q5 write a chemical equation that describes how the buffer solution neutralizes the added NaOH. What is the pH of a 100 ml. sample of distilled water at 2? degrees Celsius? PH If 0.0100 mol of HCI is added to the 100 ml. sample of distilled water in Q8, calculate the pH of the solution. Assume no volume change occurs after mixing. PH =

Explanation / Answer

3. For a buffer pH = pKa + log([base][acid])

     Here [CH3COOH] =[CH3COONa] .

     Thus pH = pKa = 4.75

4.If HCl is added, [CH3COOH] increases and [CH3COONa] decreases.

    [CH3COONa] / [CH3COOH] will be < 1 and log([CH3COONa] / [CH3COOH]) will be < 0. Thus the new pH calculated using pH = pKa + log([base][acid])

will be lower.

5.weak acid CH3COOH , weak base CH3COO-

6.CH3COO- + H+ = CH3COOH

7.CH3COOH + HO- = CH3COO- + H2O

8.[H+] = (Kwater)1/2 = (1x10-14)1/2 = 1x10-7 M , pH = -log1x10-7 =7

9.[H+] = 0.0100 mol/0.100L = 0.1 M. pH = - log0.1 = 1

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