What is the concentration of M2+ in a saturated solution of a metal hydroxide M(OH)2 (assume Ksp = 1.8 x 10-16) in an aqueous buffer of pH = 8.3?
-The answer I got was 4.5e-5 M. Just wanted to confirm this was correct, thank you!
Given : pH = 8.3
pOH = 14 - pH
pOH = 14 - 8.3
pOH = 5.7
[OH-] = 10-pOH
[OH-] = 10-5.7
[OH-] = 2.0 x 10-6 M
Ksp M(OH)2 = [M+][OH-]2
Substituting the values of Ksp and [OH-]
1.8 x 10-16 = [M+] * (2.0 x 10-6 M)2
[M+] = (1.8 x 10-16) / (2.0 x 10-6 M)2
[M+] = 4.5 x 10-5 M
What is the concentration of M2+ in a saturated solution of a metal hydroxide M(OH)2 (assume...
Consider an amphoteric hydroxide, M(OH)2 (s), where M is a generic metal. M(OH)2(s) = M2+(aq) + 2OH- (aq) Ksp = 6 x 10-16 M(OH)2(s) + 2 OH- (aq) = [M(OH)412-(aq) Kf = 0.03 Estimate the solubility of M(OH), in a solution buffered at pH = 7.0, 10.0, and 14.0. solubility at pH = 7.0 O m M solubility at pH = 10,0 solubility at pH = 10.0 solubility at pH = 14.0
Consider an amphoteric hydroxide, M(OH)2 (s), where M is a generic metal. M(OH)2(s) = M2+(aq) + 2OH- (aq) Ksp = 6 x 10-16 M(OH)2(s) + 2 OH- (aq) = [M(OH)412-(aq) Kf = 0.03 Estimate the solubility of M(OH), in a solution buffered at pH = 7.0, 10.0, and 14.0. solubility at pH = 7.0 O m M solubility at pH = 10,0 solubility at pH = 10.0 solubility at pH = 14.0
Consider an amphoteric hydroxide, M(OH),(s), where M is a generic metal. M(OH),(s) M2+ (aq) + 2OH-(aq) M(OH),(s) + 2OH(aq) = M(OH)2-(aq) Ksp = 2 10-16 M3 Ke=0.02 M- Estimate the solubility of M(OH), in a solution buffered at pH = 7.0, pH = 10.0, and pH = 14.0. solubility at pH = 7.0 solubility at pH = 10.0 Enter numeric value solubility at pH = 14.0
Be sure to answer all parts. The pH of a saturated solution of a metal hydroxide M(OH)2 is 8.950. Calculate the Ksp for this compound. Enter your answer in scientific notation.
A student measures the OH- concentration in a saturated aqueous solution of chromium(III) hydroxide to be 3.84×10-8 M. Based on her data, the solubility product constant for chromium(III) hydroxide is
What is the concentration of hydroxide ion in a 0.130 M aqueous solution of hydroxylamine, NH,OH? What is the pH? (Ks = 1.1 x 10 (OH) - M
A student measures the OH” concentration in a saturated aqueous solution of aluminum hydroxide to be 8.52x10-9 M. Based on her data, the solubility product constant for aluminum hydroxide is Submit Answer Retry Entire Group 8 more group attempts remaining
Consider a saturated solution of La(OH)3 in 0.10 M KNO3 at 25 °C. For La(OH)3, Ksp = 2.0 x 10-21. Including activities, calculate the concentration of lanthanum ions What is the pH in this saturated solution? Again, include activities. Why is the answer in part (b) still not the pH you'd measure for an actual saturated solution of lanthanum hydroxide?!
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0. Kf=0.08. Ksp=4x10^-16.
At 25 °C, what is the hydroxide ion concentration. [OH-], in an aqueous solution with a hydrogen ion concentration of TH+1=2.3 x 10-8 M2 (OH) = M