7. What mass of sodium fluoride (MW = 41.99 g/mol) must be added to 250. mL of a0.100 M HF solution to give a buffer solution having a pH of 3.500?[Ka(HF)=7.1 x 10-4] (You MUST show your work).

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Answered: 7. What mass of sodium fluoride (MW =…

Chemistry

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4. A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 \times 10-4) with 0.10 M NaOH.a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak base? (1 point) b. Estimate the pH at the equivalence point. Will it be equal to 7, greater than 7, or less than 7? Explain. (1 point) c. What is the pH after 20.0 mL of the 0.10 M NaOH is added? Show all calculations. (3 points)
4a&b
A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4). A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?
Answer the following questions about a titration between 20.0 mL of a weak base (Kb= 4.7*10-6) and 0.150 M hydrochloric acid. A.What is the concentration of the weak base solution if it requires 26.67 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of bruhmophenol is ~ 4.9 and the pKa of thymol blue ~ 9.2. Which indicator would be best to use in the titration
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A buffer is prepared by mixing 25 mL of 0.10 M nitrous acid (HNO2) and 25 mL of 0.15 M sodium nitrite (NaNO2). The Ka for nitrous acid is 5.6 x 10-4. a.) What is the pH of the buffer solution? b.) What is the pH change when 5 mL of 0.10 M HCl is added to the solution?
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A buffer solution contains 0.201 M CH3NH3 Br and 0.486 M CH3NH2 (methylamine). Determine the pH change when 0.115 mol HBr is added to 1.00 L of the buffer. (Assume Kb (CH3NH₂) = 4.2 × 10-4.) pH after addition change = Submit Answer - pH before addition = pH Retry Entire Group 9 more group attempts remaining D
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7. What mass of sodium fluoride (MW = 41.99 g/mol) must be added to 250. mL of a 0.100 M HF solution to give a buffer solution having a pH of 3.500? [Ka(HF)=7.1 x 10-4] (You MUST show your work).