Fill in the fractions required to determine the concentration of HCI. ( A ) L NaOH × ( B ) ( C 1 L NaOH (D 1 E) L HCI

(a) Ionic Solids do not dissolve in non-polar solvents. (TRUE OR FALSE) (b) H3AsO4 is a weak acid. (TRUE OR FALSE) (c) Once a chemical reaction has come to equilibrium, the reaction comes to a complete halt.(TRUE OR FALSE)

What is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base  CH3NH3Cl(aq) + NaOH(aq) ->

(a) Hydrogen peroxide, H2O2, is a Brønsted Lowry acid. It is used as an antiseptic and bleaching agent. Write the formula for the conjugate base of hydrogen peroxide.   (b) Hydrazine, N2H4, is a Brønsted-Lowry base used as a rocket fuel. Write the formula for the conjugate acid of hydrazine.   (c) Phenol, HOC6H5, is a Brønsted-Lowry acid used to make plastics, nylon, and slimicides. Write the formula for its conjugate base.   (d) Aniline, C6H5NH2, is a Brønsted-Lowry base used to make polyurethane. Write the formula for its conjugate acid.

What is the concentration (molarity) of HClO in a solution that is 0.168 M LIClO at 25°C?

(a) Calculate the OH¯ concentration in an aqueous solution at 25°C with an H3O™ concentration of 1.03 x 10 M. х 10 M (b) The value of K, at 50°C is 5.48 × 10¬14. Calculate the OH¯ concentration from the above solution at 50°C. x 10

Calculate the [OH-] in each of the following solutions: (a) [H+] = 4.0 × 10-9 [OH-] =    × 10   (b) [H+] = 1.2 × 10-5 [OH-] =    × 10     (c) 1.25 M HCN [OH-] =  x 10   M   (d) 0.333 M NaOH[OH-] =

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions. (a) CsBr;  (b) Al(NO3)3;  (c) KCN;  (d) CH3NH3Cl

(a) Calculate the H3O™ concentration in an aqueous solution at 25°C with an OH concentration of 2.00 x 10 2 M. x 10 (b) The value of K at 100°C is 5.13 × 10¯13. Calculate the H20† concentration from the above solution at 100°C. x 10