Suppose 5.00 g of propanoic acid (HC3H5O2) is dissolved in enough water to yield 100.0 mL of solution. For lactic acid, Ka = 1.3 x 10^-5. (a) Calculate the % dissociation, [H+], and pH for this solution. (b) Suppose 100.0 mL of water is added to this solution in (a). Calculate the % dissociation, [H+], and pH.

(b) CaCl2, (c) HNO3, (d) KCN, (e) Mn²+, (f) MnO4 . Calculate the pOH and pH of a 0.0045 M solution of NaOH.

Which pair of chemical species is NOT a conjugate acid-base pair? A) H,CO, and Co, В) ОН аnd Н,О C) HPO and PO, D) CH3NH, and CH,NH - When equal molar amounts of these oxides are each mixed in the same volume of water, which forms a solution with the lowest pH? A) CaO В) СО C) SỐ2 D) SO, 2. Aqueous solutions of equal molar concentrations of these salts are listed in order of increasing pH. NaBr < NalO, < NaF < NaC,H;O2 < Na,SO3 Which acid is the weakest? A) HBr B) HIO3 C) HF D) NaHSO3

In order to determine the Ka of HXO₂, a scientist prepared a HXO₂ solution with a pH=3. If the scientist determined the Ka to be 1.2 X 10⁻⁵, what was the molarity of the acid he started with? (If you use any assumptions, be sure to check that they are valid!)  Round the final answer to the three decimal places.

If 15.0 mL of glacial acetic acid (pure HC2H3O2) is diluted to 1.50 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g>mL.

In the following reaction in an aqueous solution, identify (a) which of the reactants is acid and which is the base, (b) the conjugate base of the acid, and (c) the conjugate acid of the base. NH2OH + HCl --> NH3OH+ + Cl-

HCIO is a weak acid (Ka=4.0*10^-8) and so the salt NaCIO acts as a weak base. What is the pH of a solution that is 0.018 M in NaCIO at 25 Celsius.

a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺], [OH⁻], and pH in a solution with a pOH of 4.33?

Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.

Be sure to answer all parts. Calculate the pH of each of the following solutions. (a) 3.3 x 10 M Ba(OH)2: × 10 (Enter your answer in scientific notation.) (b) 4.7 × 104 M HNO3: