Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the dry texture of certain wines. Tartaric acid, H₂C4H406, is a diprotic acid with the following Ka values: Ka1 = 1.00 x 10-3; Ka2 = 4.60 x 10-5 a. Write the equation for the 1st ionization of tartaric acid. b. Write the equation for the 2nd ionization of tartaric acid. c. Write the Ka expression for the 1st ionization.

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"

Q6

A solution with a pOH of 10.70 has an [H +] of a.2.0 × 10−12 M. b.5.0 × 10−4 M. c.3.2 × 10−4 M. d.0.36 M. e.5.0 × 10−3 M.

2. a. What is the pH of a 0.1 M solution of acetic acid? (Ka = 1.76 x 10^-5) b. Which solution is more acidic: 0.1 M acetic acid or 0.1 M HCl c. Why do these two solutions have different acidities?

Using the following K, values, calculate the pH values for each of these solutions (using 2 significant figures). [K, for acetic acid= 1.78x105; K, for phosphoric acid = 7.52x103K, for H₂CO3 = 4.3x107] A. A solution of 0.3 M acetic acid has a pH of B. A solution of 3 M acetic acid has a pH of i C. A solution of 100 mM phosphoric acid has a pH of D. A solution of 43 mM H₂CO3 has a pH of

A solution has a pOH of 4.5. What is the concentration of H3O+ in the solution in Molarity? Group of answer choices 0.0000316 M 0.00000316 M 0.00316M 3.16 x 10^-10 M 3.16 x 10^-11 M 3.16 x 10^-13 M

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. C5H;NHI 2- + 2+ 3+ 4+ 1 2 3 4 6. 7 8 9 1 3 04 O6 O7 + (s) (1) (g) (aq) C OH H. NR H2O H30* N Reset • x H2O Delete LO 3.

The concentration of hydroxide ion in an aqueous solution at 25°C is 7.2 x 10-4 M. What is the concentration of the hydronium ion? 1 2 3 4 6. C 7 8 9. +/- x 100 +

Carbonic acid, H2CO3, can be found in a wide variety of body fluids (from dissolved CO2). Calculate the hydronium ion concentration of a 3.04 x 10 M H2CO3 solution. What is the concentration of CO3? K, = 4.3 x 107 Ka, = 4.8 x 10-11 zasa