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[C6H6O62-] = M.
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- Calculate the concentration of HC6H₂O6 in an aqueous solution of 0.0337 M ascorbic acid, H₂C₁H₂O6 (aq). [HC6H6O6 ] = M.The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 MDetermine 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. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.
- 6. (i) Define pH in words. The strong acid HClag has a pH value of 1, use the following equation for a strong acid: HClaa Hog + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] Clea (ii) Use the above expression to deduce the pH of HCl (ag) given the concentration of the acid to be 4.5 mol/dm³ pH =What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =
- 8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.6. (a) Aspirin is a weak acid with a pKa of 3.6 and MW 180 g/mol. The saturation solubility (S) of aspirin in water is 3.3 g /L and a saturated solution has pH equal to your answer to question 4(b) above. What is the solubility of the unionised form (So) of aspirin at this pH using units of mol/L and g/L. (b) Use the So value (just obtained) to calculate the saturation solubility (S) of aspirin in water at pH 6.6 using units of mol/L and g/L. (c) If you modified the aspirin suspension APF12 formula by replacing the purified water with pH 6.6 buffer, would the product be a suspension or solution?
- A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.Calculate the hydronium ion concentration in an aqueous solution of 0.198 M carbonic acid, H,CO3 (aq). [H;O"]=[ M.According to Henry’s law the atmospheric partial pressure of CO2 dictates the concentration of aqueous CO2 according to the following equilibrium expression where k is the Henry’s law constant for CO2. CO2 (g) <-> CO2 (aq) k=1x10^-1.5 The acid dissociation constant Ka for carbonic acid applies to CO2 (aq). Given pKa1=6.35 and pKa2=10.33 and the fact that the partial pressure of CO2 in the atmosphere is 10^-3.5 atm, find the pH of water in equilibrium with the atmosphere.
