A biochemist has a 100 mL of a 0.1 M solution of a weak acid with a pKa of 6.3. She adds 6 Ml of 1.0 M HCL, which changes the pH to 5.7. Calculate the pH of the original solution.
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A biochemist has a 100 mL of a 0.1 M solution of a weak acid with a pKa of 6.3. She adds 6 Ml of 1.0 M HCL, which changes the pH to 5.7. Calculate the pH of the original solution.
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- A biochemist has 100 mL of a 0.10 M solution of a weak acid with a pKa of 6.3. She adds 6.0 mL of 1.0 M HCl, which changes the pH to 5.7. What was the pH of the original solution?Describe how you would prepare a 500 ml of 0.35M Glycine pH2.2 from a 5M Glycine solution of pH 7. Show your calculations.kindly answer the first question, show the full solution.
- A volumetric flask is made to prepare a certain chemical concentration through dilution for example if there is no volumetric flasks how can you prepare 0.2N or acetic acid from 1 N acetic acid stock solution.A 25.00 mL sample of 0.320 M LIOH is titrated with 0.750 M HNO3 at 25 °C. Calculate the initial pH before any titrant is added. pH = Calculate the pH of the solution after 5.00 mL of the titrant is added. pH =Give Detailed Solution (don't give Handwritten answer.
- What is the approximate pH of a solution labeled 6 x 10-5 M HBr? * 4.2 4.5 5.8 9.8 8.2A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units unitsThe pKa values of a compound with two ionizable groups are pK1 = 4.10 and pK2 between 7 and 10. A biochemist has 10 mL of a 1.0 M solution of this compound at a pH of 8.00. She adds 10.0 mL of 1.00 M HCl, which changes the pH to 3.20. What is pK2?
- A beaker with 1.40x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.00 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( - ) sign if the pH has decreased. View Available Hint(s) ΑΣφ ApH =A 0.200 M solution of a weak monoprotic acid (HA) has a pH of 2.35. What is the value of K of this acid? a K =2.011e-4 a What is the percent ionization of this acid? Percent Ionization = .10 %80.00 mL of 0.350 M benzoic acid (K = 6.4×105) is titrated by 0.350 M NaOH. Calculate the pH of the acid solution before any titrant is added. PH Calculate the pH after 58.9 mL of 0.350 M NaOH is added to 80.00 mL of 0.350 M benzoic acid. pH = Calculate the pH after 80.00 mL of 0.350 M NaOH is added to 80.00 mL of 0.350 M benzoic ad pH = Calculate the pH after 110 mL of 0.350 M NaOH is added to 80.00 mL of 0.350 M benzoic acid. pH=