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: Kal = 1.00 x 10-3; K₁2 = 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.

Given the value of Kw = 1.0 × 10^-14 at 25 °C.a. Write the relevant chemical reaction.b. Calculate the molarity of OH^- in a solution where the concentration of H+ is 0.4 M at 25 °C.c. Calculate pOH for this solutiond. At 40 °C the ionization constant for water (Kw) is 2.9 × 10^-14. Calculate [H3O^+], [OH^−], pH, and pOH for pure water at 40 °C.

5. What amount of solid NaOH must be added to 1.0 L of a 0.12 M H2CO3 solution to produce a solution with [H+]= 3.1x10-11 M ? There is no significant volume change as the result of the addition of the solid.

For the reaction below: which base(s) (I – V) will have an equilibrium constant greater than 1 Base + H-Base + Base = H H O. Na H. II IV V O Iv O I, III, IV O 1,II II O II, V 00

Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the dry texture of certain wines. Tartaric acid, H2C4H4O6, is a diprotic acid with the following Ką values: Ka1 = 1.00 x 10-3; Ka2 = 4.60 x 10-5 a. Write the equation for the 1st jonization of tartaric acid. b. Write the equation for the 2nd ionization of tartaric acid. c. Write the Ką expression for the 1st ionization. d. Write the Ką expression for the 2nd ionization. e. What is the equilibrium concentrations of the reactants and products from the 1st ionization of a 0.250M solution of tartaric acid? f. What is the equilibrium concentrations of the reactants and products from the 2nd ionization? g. What is the total [H30+] and the overall pH of the solution of tartaric acid?

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. CSHSNHI 04- D2+ 3+ 4+ 1 2 4 5 7 9 3 Os (s) (1) (g) (aq) + OH- NR H H3O+ C H2O Reset • x H2O Delete CO LO

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; K₁2 = 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. d. Write the Ka expression for the 2nd ionization. e. What is the equilibrium concentrations of the reactants and products from the 1st ionization of a 0.250M solution of tartaric acid? f. What is the equilibrium concentrations of the reactants and products from the 2nd ionization? g. What is the total [H3O+] and the overall pH of the solution of tartaric acid?

Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI

Calculate the [H† of a solution at 25 °C that has a p)H = 5.43. Type your answer...

What is the ratio of bicarbonate ion to carbonic acid ([HCO−3]/[H2CO3])([HCO3−]/[H2CO3]) in blood serum that has a pHpH of 7.40?  Express your answer using three significant figures.