A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.11 mol of ma

ID: 580601 • Letter: A

Question

A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.11 mol of magnesium nitrate in water to give 1.00L of total volume. Ka= 4.5*10^-4

1. What is the pH of the resulting solution? (I already calculated this to be 3.03 and would like to know if I'm correct.)

2. When 0.010 mol HCl is added to this solution, the pH will:

a. Increase slightly

b. Decrease slightly

c. Not change

d. More information is needed

3. What will the new pH be after the addition of 0.010 mol NaOH?

a. 7.00

b. 12.0

c. 3.61

d.3.09

pKa = -log Ka

pKa = 3.35

1. What is the pH of the resulting solution

pH = 3.03 your answer is correct

2) answer b. Decrease slightly

new pH

pH = pKa + log [salt + base moles / acid - base moles]

pH = 3.35 + log (0.11 + 0.01 / 0.23 - 0.01)

pH = 3.09

answer is d) 3.09

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