SECTION 2 Work out the following problems on separate sheets in the same or how
ID: 1041518 • Letter: S
Question
SECTION 2 Work out the following problems on separate sheets in the same or how all work clearly. Correct answers without work will not be given full credit. the same order as the questions I. Hydroxylamine (NH OH) is an organic base. A 0.15 M solution of hydroxylamine has a (10 points) 2. HC?O has a K, of 3.5 x 10", what molarity of HCIO is required to produce an aqueous (12 points) 3, what is the pH of a 0.25M KCN solution? K, for HCN-1.0 x 10'0 (14 points) pH of 10.11. What is the Ke for this base solution with a pH of 3.10? 4. What is the pH of the resulting solution when 30.00mL of 1.50M NaOH has been added (12 points) to 50mL of 0.45M HCl? 5. Calculate the solubility of Fe(OH)s at 25°c. Kip of Fe(OH) 1.1 x 103 (8points) 6. A 0.15 M solution of a weak acid (HF) has a pH of 3.28. (8 points) a) What is the percent ionization of this acid? b) What is the Ka and pKa of this acid? How many moles of HNO, must be added to 0.200M NaNO2 to give a 2.00L of a solution with pH 4.20? Assume no change in volume occurs due to the addition of HNO2. (Ka for HNO2 4.1 x 104) 7. (10 points) 8. If 135mL of 0.15M BaClh is mixed with 75mL of 0.001M Na SO, will a precipitate form? Ksp for BaSO, 1.1 x 1010 NH20H I 15 Some Useful Formula 1. For Buffer Solutions Only pH pK +log(ISalt/[Acid]) pOH-pKb + log(ISalt/IBase]) 15Explanation / Answer
2.
pH = -Log[H3O+]
- Log[H3O+] = 3.10
[H3O+] = 10-3.10
[H3O+] = 0.000794 M
According to Ostwald's theor of weak electrolytes,
[H3O+] = sqrt.(Ka*C)
0.000794 = sqrt.(3.5 * 10-8 * C)
C = Molarity of HOCl = 18.0 M
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