Consider a dihydrogen phosphate buffer at pH = 7.20.  Which species would react if an external base , OH- were added? a. H2PO4- b. H3PO4 c. HPO4^2- d. PO4^3-

a. A hydrochloric acid solution has a pH value of 3. Which of the following substances would increase the pH value of the solution when mixed with it? (1) Dilute ammonia solut(2) Dilute (3) WaterA(1) and (2) onlyB(1) and (3) onlyC(2) and (3) only D 1,2,3   b. Which of the following statements about a concentrated acid is correct?A. It can react with copper metal.B. It cannot react with copper(II) oxide.C. It is an acid that fully ionizes in water.D. It must contain hydrogen ions when in aqueous form. c. which of the following states of hydrogen chloride will not turn dry blue litmus paper red? (1) HCl gas(2) HCl in water(3) HCl in methylbenzene (an organic solvent)A. (1) onlyB. (2) onlyC. (1) and (2) onlyD. (1) and (3) only

Calculate the pH of a buffer solution made by dissolving 50 g of NaHCO3 and 20 g of H2CO3 to make 100 mL of a buffer solution. Help! H2CO3 Ka1= 4.30 x 10^-7 a. 6.77 b. 6.63 c. 6.10 d. 6.37

number 5 please!

2. Which of the following will NOT work as a buffer pair? A. ΝH3/ΝH4Br B. HBr/KBr C. HCIO/NaCio D. CH3COOH/NaCH3COO

7. Consider a buffered solution at a pH of 4.00 made with HF (K₁ = 7.2 x 104) and NaF. Which of the following statements is true? Assume all of the concentrations below refer to equilibrium concentrations. A) [HF] = [F] B) [HF] = [H*] C) [HF] > [F] qme D. [H¹] = [F] E. [HF] [F]

Help please

2. Let's prepare an H₂SO4 solution by dissolving 4.9 grams of H₂SO a. How man b. is the molarity of the solution? is the pH of the solution? C. Wr H₂SO4 molecules are in this solution? d. Wir her is datin ފނމފރ ހރތ **S in 100 mL of water. pH of the solution if adding 3.0 grams of NaOH to the solution?

3. Calculate the pH of the following aqueous solutions. a. 2.62 x 10-1 M HCl b. 9.6 x 10-12 M HNO3 c. 5.00 mL’s of solution a. diluted to 100.0 mL in a volumetric flask.

Match each compound with the word or phrase that best describes it. Fe(OH)2 ✓HCIO ✓HSO4 ✓ HBr OH™ A. Strong electrolyte B. Arrhenius base C. proton acceptor D. Weak electrolyte E. Can behave as both an acid or a base