(References) A typical vitamin C tablet (containing pure ascorbic acid, H2C6H606) weighs 500 mg. One vitamin C tablet is dissolved in enough water to make 250.0 ml of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid, For H2C6H606, Kal 7.9x10-5 and Ka2 1.6x10 12 pH =

Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215 mol/L H2NNH3Br solutionGive an answer to at least 3 decimal places. Next, calculate the pH of this same solution if 12.00 mL of 0.300 mol/L HNO3 is added.Give an answer with at least 3 decimal places.

The pH of a 0.56M solution of hexanoic acid (HCH0,) is measured to be 2.55. Calculate the acid dissociation constant K, of hexanoic acid. Be sure your answer has the correct number of significant digits. K. = 0 -10 The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10 . a Calculate the pH of a 0.42M solution of boric acid. Round your answer to 1 decimal place. pH =

The acid dissociation constants for phosphoric acid (H₂PO4) are Kal = 0.00711, Ka2 = 6.32 x 10-8, and K₁3 = = 7.1 x 10-13. Determine whether a solution made by dissolving KH₂PO4 in water is acidic, basic, or neutral. O acidic not enough information basic neutral

Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid 0.1 M KCI acid solution 0.1 M KCIO 0.1 M C6H5NH3Br 0.1 M NH4CI formula HCH3CO₂ 1.8 x 10-5 HCIO Ra Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 3.0 × 10 pH choose one -8 choose one choose one base choose one ✓ Ko name formula aniline C6H5NH₂ 4.3 × 10¯ - 10 ammonia NH3 1.8 × 10

Determine [OH–], pOH and pH of a 0.63 M  aqueous solution of LiC3H5O3 (K b = 7.1×10-11).

Consider the following data on some weak acids and weak bases: acid base Ka Kb name formula name formula - 10 4.9 x 10 4 hydrocyanic acid HCN methylamine | CH3NH, | 4.4 x 10 C,H;NH2 4.3 × 10 HNO, 4.5 x 10 - 10 4 nitrous acid aniline Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М КCN 4 (highest) 0.1 M C6H5NH3Br 1 (lowest) 0.1 M NaNO2 3 0.1 М KBr 2

For the diprotic weak acid H2A, ?a1 = 2.3×10−6 and ?a2  = 6.8×10−9. What is the pH of a 0.0500 M solution of H2A? pH=     What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]=                                                       M     [A2−]=                                                        M

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For the diprotic weak acid H2A, Kal = 2.4 × 10-6 and Ka2 What is the pH of a 0.0700 M solution of H₂A? pH = 10.96 = 8.0 × 10-9. What are the equilibrium concentrations of H₂A and A²¯ in this solution? [H₂A] = [A²-] = M M