What is the pH of a 0.55 M solution of Al(H2O)3+6 if the Ka for the hydrate is 1.4×10−5?
What is the pH of a 0.55 M solution of Al(H2O)3+6 if the Ka for the...
Find the pH of a 0.008 M solution of an aluminum compound which dissolves completely to give the hydrated aluminum ion Al(H2O)3+6. Al(H2O)3+6(aq)+H2O(l)⇌H3O+(aq)+Al(H2O)5(OH)2+(aq), Ka=1.4×10−5 Report your answer with three significant figures. Find the pH of a 0.008 M solution of an aluminum compound which dissolves completely to give the hydrated aluminum ion Al(H2O)3+6. Al(H2O)3+6(aq)+H2O(l)⇌H3O+(aq)+Al(H2O)5(OH)2+(aq), Ka=1.4×10−5 Report your answer with three significant figures.
Calculate the pH of a 2.55 M solution of FeCl3. (Fe(H2O)6^3+, Ka=6.3x10^-3)
2. Calculate the pH of a 0.10 M solution of aluminum chloride, which dissolves completely in water to give the hydrated aluminum ion [Al(H2O).]* in solution. Al3(aq) + H2O + [Al(H2O)]3+(aq) (Al(H20)6]3(aq) + H2O(0) [Al(H20)SOH)2(aq) + H3O(aq) Ka = 1.4 x 10
The weak acid HA has a Ka of 4.5×10−6. If a 1.4 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HA(aq)+H2O(l)⇋H3O+(aq)+A−(aq)
What is the pH of a 6.85 × 10−3 M weak acid solution, HA, if Ka = 4.5 × 10−6? Group of answer choices 1.2 4.8 9.1 3.8 6.5 What is the pOH of 4.50 × 10−4M HBr? Group of answer choices 10.7 6.7 1.7 12.3 3.3 What is the pH of a 9.67 × 10−3M solution of NaOH? Group of answer choices 13.0 4.6 12.0 9.4 2.0 A 6.5 × 10-2 M solution of a weak acid, HA, has...
The pH of a 0.10 M solution of hydrazoic acid, HN3, is 2.86. Calculate the Ka value for hydrazoic acid. A. 1.4 x 10-4 B. 1.9 x 10-5 C. 1.9 x 10-3 D. 1.4 x 10-5 E. 2.6 x 10-3
Q: What is the pH of a solution containing 0.125 M KH2PO4 and 0.175 K2HPO4 Ka (H2PO4-) = 6.2 x 10-8 Ka (HPO42-) = 4.8 x 10-13 Q: A 0.15 M solution of a weak acid is 3.0 % dissociated. What is the Ka of this acid? Q: A solution of aspirin was prepared that is 0.16 M. The pH of this solution was measured to be 2.43. What is the Ka of aspirin? Q: A solution of formic acid...
Al(OH)3 + 3 H+ <--> Al3+ + 3 H2O You find that the solution pH = 5, and that [Al3+] = 10-2 mol/L. Assuming the activity coefficient = 1 for Al3+, what is the log(Keq) of the Al(OH)3 dissolution written above assuming the system is at equilibrium? If you got stuck on a, assume that log(Al3+)=log(Keq)-3pH + 30.
Calculate the pH of a 0.0208 M sodium chloroacetate solution. Ka (HC2H2O2Cl) = 1.4 × 10−3. Report your answer to TWO places past the decimal.
1. What is the Kb for B-, if the Ka for the acid (HB) is 2.5 x 10-8? 2. What is the hydronium ion concentration of a 3.50 x 10-2 M solution of the monoprotic acid, HBrC6H4COO, for which Ka = 1.00 x 10-4? 3. What is the Ka value for HB, if a solution that is 0.25 M B- and 0.55 M HB produces a pH of 4.95? 4. Calculate the pH of a solution containing .225 moles of...