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- The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.Given three acid-base indicators—methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)—which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid1: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中
- (a) Determine the pH of a buffer containing 0.12 M acetic acid (pKa = 4.76) and 0.078 M sodium acetate? (b) For 1.00 L of the buffer in part (a) of this question, estimate its buffer capacity if 14 mL of 1.0 M HCl is added to the buffer. (c) Calculate buffer capacity using the van Slyke equation and compare this value with the buffer capacity determined in part (b) of this question. (d) (i) Calculate the pH of a 55 mg mL-1 solution of ascorbic acid (pKa = 4.17, M = 176.1 g mol-1). (ii) What is the degree of ionization (in %) of a 55 mg mL-1 solution of ascorbic acid at a pH of 2.0 and at a pH of 7.0? (iii) Briefly explain how the differences in ionization values arise between these two pH values. (e) A 5% w/v solution of lignocaine hydrochloride (M = 270.79 g/mol) is prepared. The solubility of lignocaine (M = 234.34 g/mol), a weak organic base (pKa = 7.95 and M = 234.33 g/mol) is 3.81 mg/mL. Calculate the pH at which lignocaine will begin to precipitate out of this solution.A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and 0.30 molmol of NH4ClNH4Cl. What mass of the correct reagent should you add? Express your answer using two significant figures.A 65.0 mL solution of 0.158 M potassium alaninate ( H,NC, H,CO, K) is titrated with 0.158 M HCI. The pK values for the amino acid alanine are 2.344 (pKa1) and 9.868 ( CH3 pKa2), which correspond to the carboxylic acid and amino H2N CH-C- groups, respectively. Calculate the pH at the first equivalence point. Potassium Alaninate pH = %3D Calculate the pH at the second equivalence point. pH =
- A buffer solution contains 0.384 M KHCO3 and 0.239 M Na₂CO3. If 0.0464 moles of potassium hydroxide are added to 225.0 mL of this buffer, determine the pH of the resulting solution. Assume that the volume does not change upon adding potassium hydroxide. Given K₂ of HCO3¯ = Ka2 of H₂CO3 = 4.7 x 10-11How many grams of sodium acetate (salt) and acetic acid (acid) would be required to prepare 1 L of acetate buffer with a total buffer concentration of 0.6 moles/litre, given a mole fraction of salt (Xsalt) and acid (Xacid) of 0.75 and 0.25, respectively? [The molecular weight of sodium acetate (salt) is 82 g/mole and the molecular weight of acetic acid (acid) is 60 g/mole]. O a.sodium acetate = 110.7 g; acetic acid = 51 g b. sodium acetate = 27 g; acetic acid = 12.3 g O c. sodium acetate = 29 g; acetic acid = 5.5 g d. sodium acetate = 36.9 g; acetic acid = 9g O e. sodium acetate = 12.3 g; acetic acid = 9 gDetermine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka for CH3COOH is 1.8 x 10-5. Complete Parts 1-3 before submitting your answer. 3 NEXT > The buffer was prepared by dissolving 20.0 g NaCH3COO into a 500.0 mL solution of 0.150 M of CH3COOH. Assume the volume of the solution does not change. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 1 CH3COOH(aq) 0.150 -X 0.150 - x + 2 H₂O(l) H3O+ (aq) 0 +x +x + CH3COO-(aq) 0.488 +x 0.488 + x
- 100 mL of a benzoic acid (C5H6COOH) buffer solution is made with initial concentrations of [C5H6COOH] = 0.33M and [C5H6COONa] = 0.28M. The Ka of benzoic acid is 6.3x10-5. a) What is the pH of the buffer solution initially? b) What is the pH of the buffer after the addition of 0.5g NaOH(s). c) What minimum volume of 1M HCl should be added to exceed the buffer capacity of this solution (the buffer capacity is reached when one component of the buffer is less than 10% of the other) d) How could this initial buffer be created by combining solutions of HCl and C5H6COONa? (No calculation needed, just a detailed qualitative answer)A 45.0 ml sample of 0.456 M ascorbic acid, HC6H;O6, was titrated with 0.332 M KOH solution. Ka = 8.0 x 10s a. Using an ICE box and balanced chemical equation show the number of moles of each substance at equilibrium after 20.0 mL of KOH was added to the ascorbic acid. Spectator ions should be left out of the equation. b. Explain why the mixing of 45.0 mL of 0.456 M ascorbic acid and 20.0 mL of 0.332 M KOH resulted in the formation of a buffer? C. Determine the pH after the addition of 75.0 mL of 0.332 M KOH to 45.0 mL of 0.456 M ascorbic acid solution.You want to make a 500.0 mL of 0.0500 M of phosphate buffer pH = 6.80 from solid Na2HPO4 compound and a 0.300 M of NaH2PO4 solution on the shelf. Calculate the mass of solid Na2HPO4 compound required and calculate the volume of the 0.300 M of NaH2PO4 solution required to make the buffer, then explain briefly how you would make the buffer. You will need the Molar Mass of Na2HPO4. Ka of NaH2PO4 = 6.2 x 10-8. Note: the [Na2HPO4] + [NaH2PO4] = 0.0500 M.