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- 9. 1.4 g of glucose (C6H1206) is dissolved in 150 ml of water (final volume). What is the final number of moles and the molarity of the solution?What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4A solution with a density of 0.876 g>mL contains 5.0 g of toluene 1C7H82 and 225 g of benzene. Calculate the molarity of the solution.
- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.What is the molarity of a NaOH solution if 48.0 mLneutralizes 35.0 mL of 0.144 M H2SO4?Calculate the pH of a solution that is 0.05000 M NH4Cl and 0.0300 M NH3 (Kb for NH3 = 1.8 x 10-5)
- If 10x TBE contains 0.89 M Tris-borate, 0.89 M Boric acid, and 0.02 M EDTA, what is the Molar concentration of Tris-borate in 100 ml of 1x TBE?Calculate the normality of a solution that contains 4.5 g of (COOH)2 in 3000 mL of solution? (Assume the (COOH)2 is to be completely neutralized in an acid-base * reaction.) 0.033 N O 0.33 N O 0.166 N O 0.0166 N 0.45 N O 0.045 N 000.0 OOConsider the following acids and their ionization constant, determine which conjugate base is HCOOH Ka = 1.7 x 10-4 (b) HCN Ka = 4.9 x 10-10
- 4.2 (b) Using the equation below, explain what happens to maintain the pH of the solution: A (aq) H(aq) HA (aq) (i) when an acid is added (ii) when a base is added (iii) Give one example each of a buffer in both living and non-living systems +Titration of a 12.0 mL solution of HCl requires 22.4 mL of 0.12 M NaOH. What is the molarity of the HCl solution?The solubility product of a metal hydroxide M(OH)2 is 8.65 × 10-6. What is the molar solubility of the M(OH)2 in a buffer solution of pH = 13.3?