Calculate the hydrogen ion concentration in a solution having a pH of 4.60. 4.0

Question

Calculate the hydrogen ion concentration in a solution having a pH of 4.60. 4.0 times 10^-3 M 4.0 times 10^-9 M 4.0 times 10^-10 M 2.5 times 10^-5 M 2.5 times 10^-4 M The solubility product for chromium(III) fluoride in K_sp = 6.6 times 10^-11. What is the molar solubility of chromium (III) fluoride? 1.6 times 10^-3 M 1.2 times 10^-3 M 6.6 times 10^-11 M 2.2 times 10^-3 M 1.6 times 10^-6 M Select True or False: The ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO_2/HNO_2 buffer is correctly shown here: OH^- + HNO_2 rightarrow NO_2^- + H_2O True False Which of the following yields a buffer solution when equal volumes of the two solutions are mixed? 0.10 M H_2CO_3 and 0.050M HCI 0.10M H_2CO_3 and 0.10 M KOH 0.10M H_2CO_3 and 0.10 M HCI 0.10M H_2CO_3 and 0.050M KOH 0.10 M K_2CO_3 and 0.050M KOH Calculate the pH of a 1.6 M KOH solution. 1.60 -0.20 0.20 14.20 13.80 You have 500.0 mL of a buffer solution

Explanation / Answer

7)
pH = -log [H+]
4.60 = -log [H+]
[H+]= 2.5*10^-5 M

Answer: D

8)
CrF3 <--------> Cr3+ + 3 F-
s 3s

Ksp = [Cr3+] [F-]^3
6.6*10^-11 = s*(3s)^3
6.6*10^-11 = 27*s^4
s = 1.2*10^-3 M

Answer: B

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