Which one of the following values of [OH-] and pH is correct? A. 1.50 g of LiOH in 250. mL of solution has [OH-] = 0.251 M and pH = 0.601 B. A solution formed by adding 5.00 mL of 0.0105 M KOH to 15.0 mL of 3.5 x 10-3 M Ca(OH)2 (assume that the volumes of the solutions are additive) has [OH-] = 7.9 x 10-3 M and pH = 11.90. C.1.00 mL of 0.095 M NaOH diluted to 2.00 L has [OH-] = .0495 M and a pH = 12.7 D. 3.5 x 10-4 M Sr(OH)2 has [OH-] = 7.0 x 10-4 M and pH = 3.15 The answer is B.

Help please

8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HClO2, is a moderately strong acid with a Ka 1.110×10-². Please answer the following questions. A. = B. What is the molarity of the HClO2 solution whose pH is 2.38? M Please provider your answer below. 3.76E-5 Check answer A 仁 To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HClO2 is 0.6013 M? M Please provider your answer below. 0.₂ Check answer → $ $

A solution is prepared by dissolving 1.500 g of sodium acetate (CH3COONA) into 100.00 mL of a 0.150 M solution of acetic acid. The K, of acetic acid is 1.8 × 10. What is the pH of the solution? pH = %3D

Consider the following reaction at equilibrium. CH,COOH(aq) = CHyco0 (aq) + H*(aq) When NaCH3CO0 is added to the solution will the value of the equilibrium constant, K, and the pH of the solution increase, decrease, or remain the same? Select one: O A. K, decreases and pH increases O B. Ka remains the same and pH decreases O C. Ka decreases and pH remains the same O D. K, remains the same and pH increases O E. K, increases and pH decreases

Each solution below has pH = 4.5. Which solution most effectively maintains pH between 4.0 and 5.0 upon addition of a small amount of strong acid or base? O 1.00 M NaF +0.050 M HF. K₂(HF) = 6.3 x 10-4 O 2.1 M NaH₂PO4 + 0.0085 M H3PO4. Ka1(H3PO4) = 7.5 × 10-³ 0.80 M NaNO₂ + 0.055 M HNO₂. Ka(HNO2, nitrous acid) = 4.6 x 10-4 O 1.0 M NaC7H502 +0.50 M HC7H5O2. Ka(HC₂H5O₂, benzoic acid) = 6.3 × 10-5

What is the pH of the solution that results from adding 24.7 mL of 0.11 M HCl to 25.2 mL of 0.41 M NH3 ? (K, for ammonium ion is 5.6 x 10-10 ) pH =

H8. What is the pH of an aqueous solution made by combining 43.55 mL of a 0.3692 M ammonium chloride with 42.76 mL of a 0.3314 M solution of ammonia to which 4.743 mL of a 0.0752 M solution of HCl was added?

Please answer only part D of this question. Thanks

A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? pH B. What is the hydroxide ion concentration, [OH], in an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.190 M, [H*] = 4.00 x 104 M, and [A-] = 4.00 x 104 M. Calculate the Ką value for the acid HA. Ka = TOOLS x10"