11. What is the pH of 6.5 x 10' M KOH(aq) at 25 °C?(K - 1.01 X 10-) a. 4.19 b. 1.54 c. 4.19 d. 9.81 e. 12.46
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of a 0.10 molar solution of sodium cyanide, which contains the cyanide ion? a. 5.10 b. 8.90 c. 9.21 d. 11.10 e. 11.30 9. The solubility product for Ag3PO, is: Kop = 2.8 x 101 What is the solubility of Ag,PO, in water, in moles per liter? a. 1.8 x 10M b. 2.5 x 10M c. 1.9 x 10 M d. 3.1 x 10M e....
4 questions
What is the pH of egg whites with [OH-] = 1.2 x 10-5 M? A 9.08 3.4.92 C. 11.00 D. 10.50 O E. 12.08 QUESTION 26 What is the pH of an aqueous solution contains 0.0025 M of Hydroxide ion? 2.60 3.60 10.40 11.40 8.40 A 30. mL of a 0.50M solution of NaOH is titrated with 0.50M HNO3. Calculate the pH of the solution after 30. mL of HNO3 has been added? 0.30 0.50 7.0 5.0 3.0...
What is the pH of a 8.6 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. pH = Assuming complete dissociation, what is the pH of a 3.98 mg/L Ba(OH), solution? pH = X10 Assuming equal concentrations, arrange these solutions by pH. Highest pH Lowest pH Answer Bank HCIO, (aq) Cabr,(aq) NaCN(aq) CH, NH, Br(aq) RbOH(aq)
What is pH of the 1.2 M H2SO; K1 -2.4 10-3K 2 - 4.8 10.9. 3.62 9.88 4.12 1.27
Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the pH of a solution that contains 1.0 M KNO2(aq) and 0.50 M HNO2(aq).
What is the pH of a 2.50 molar solution of NaCN(aq)? KA (HCN) = 6.2×10^-10 a. 11.80 b. 9.60 c. 9.21 d. 4.40 e. 2.20 A. is the correct answer
What is the pH of a 4.0 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. 6.53 0 pH = Consider the reaction. CH,CH,0 + HCECH =HCEC:" + CH, CH,OH Classify each reactant and product as an acid or base according to the Brønsted theory. Acid Base CH,CH,0 HCEC" HCECH CH,CH, OH Answer Bank Each value represents a different aqueous solution at 25°C. Classify each solution as acidic, basic, or neutral. Acidic Basic...
Form 1 29. Determine the pH of a 0.741 M LiOH solution at 25°C. A) 0.130 B) 13.87 C) 0.741 D) 13.26 E) 1.18 30. What is the hydronium ion concentration of a 0.500 M acetic acid solu Ka = 1.8 x 10-5? The equation for the dissociation of acetic acid is: centration of a 0.500 M acetic acid solution with CH3CO2H(aq) + H2O(1) = H30+(aq) + CH3CO2"(aq) A) 3.0 x 10-2 M B) 4.2 x 10-2 M C) 3.0...
Calculate the Ka (aq., 25 °C) of a 0.250 M weak acid whose pH is 3.86. The base-ionization constant of ethylamine (C2H5NH2) is 6.4 x 10-4 at 25.0 °C. The [H+) in a 1.6 x 10-2 M solution of ethylamine is M.