Which pair of aqueous solutions can create a buffer solution if present in the appropriate concentrations? A. HCl and H20 B. HCl and NaOH C. H3PO4 and Na3PO4 D. HF and NaF
Q: What is a buffer? a. a solution that resists change to pH b. any solution at equilibrium c.…
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Q: bläi 3 What are the buffer solutions? What ?they consist of إجابتك
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Q: 20. Which of the following pairs of solutions can form a buffer? A. 1.0 M H2SO, and 1.0 M NazSO3 B.…
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Q: 90. Which substance could you add to each solution to mal it a buffer solution? (a) 0.050 M NaHSO3…
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Q: 4.75 В. 4.80 С. 4.65 D. 4.79 ywords: buffer, neutralization, weak acid, conjugate acid, conjugate…
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
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A: To find the correct statement for a buffer: (a) Maintain neutral or pH 7.0 pH from small additions…
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Q: What is the concentration of the unknown HCl solution in M?
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Q: A buffera. slows down chemical reactions.b. speeds up chemical reactions.c. increases the pH of a…
A: Solution- A buffer - maintains a relatively constant pH. Changes the pH of acid and base solutions.…
Q: a. What concentration will result if 43.8 ml of H20 is added to 33.3 ml of 7.85 M HCI ?
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Q: Titration is a common laboratory method used to verify the concentration of a chemical. On Mars,…
A: The balanced equation for the reaction of NaOH and H2SO4 as follows; 2 NaOH + H2SO4 → Na2SO4…
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Q: 58/ Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HCIO4 c. a solution that is 0.045 M…
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Q: A solution is buffered at a pH of 6.5 and a small amount of acid is added. What happens to the pH of…
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Q: 20. Which of the following pairs of solutions can form a buffer? A. 1.0 M H2S04 and 1.0 M NaHSO4 B.…
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Q: Calculate the change in pH to 0.01 pH units caused by adding 10. mL of 2.82-M NaOH is added to 440.…
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A: #Q.15: A buffer solution is an aqueous solution that contains a weak acid/base and its conjugate…
Q: Buffers are aqueous solutions that tend to resist changes in pH when small amounts of strong acid…
A: #Q.28: A buffer solution is an aqueous solution that contains a weak acid/base and its conjugate…
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A: A buffer is a solution which resist the change in its pH upon addition of an acid or a base.
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Q: A solution is buffered at a pH of 6.5 and a small amount of base is added. What happens to the pH of…
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Q: how we can implement acid base titration in pharmaceutical industries
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Q: What does a buffer solution do?* increase the pH neutralizes excess hydrogen and hydroxyl ions…
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A: The given data contains, volume of acid = 12 ml. Volume of KOH = 36 ml Molarity of KOH =0.16 M.
Q: A solution containing which one of the following pairs of substances will be a buffer solution?…
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Q: Which of the following systems will form (a) buffer solution(s)? A.NaHSOA/H25OA B. Na2HAsOA /…
A: Buffer solution are the solutions whose pH do not change on addition of acid or base to them .…
Q: Which of the following sets of compounds, when dissolved in the same solution,. forms a buffer…
A: Correct answer is NaC2H3O2 and HC2H3O2 . Mixture having weak acid and its salt with strong base is…
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- A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the most likely value for the buffer solution pH after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?. When sodium hydroxide, NaOH, is added dropwise to a buffered solution, the _______ component of the butter consumes the added hydroxide ion.A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?
- A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of solution. The pH of the final solution is 4.56. a What is the molar concentration of the acetic acid? b How many milliliters of hydrochloric acid were added to the original solution? c What was the original concentration of the sodium acetate?Use the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.). Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.
- A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.