Consider a strong acid-weak base titration between 0.250 M HNO3 and NH3. a. The volume of HNO3 added at the equivalence point is 20.50 mL. Calculate the number of moles of HNO3 used in the titration. 5.125e-3 b. Calculate the number of moles of NH3 in the flask 5.125e-3 c. Find the concentration of NH3 in the solution, if 25.00 mL of NH3 is used in the titration. 0.205 mol L-1 d. What is the species present at the equivalence point? e. Find the concentration of the salt present at the equivalence point.| f. The Kp of NH3 is 1.8 × 10-5. What is the Ka of NH4*?| g. Find the concentration of H* at the equivalence point. h. Calculate the pH and pOH of the solution at equivalence point pH =

Consider a strong acid-weak base titration between 0.250 M HNO3 and NH3. a. The volume of HNO3 added at the equivalence point is 20.50 mL. Calculate the number of moles of HNO3 used in the titration. 5.125e-3 b. Calculate the number of moles of NH3 in the flask 5.125e-3 c. Find the concentration of NH3 in the solution, if 25.00 mL of NH3 is used in the titration. 0.205 mol L-1 d. What is the species present at the equivalence point? e. Find the concentration of the salt present at the equivalence point.| f. The Kp of NH3 is 1.8 × 10-5. What is the Ka of NH4?| g. Find the concentration of H at the equivalence point. h. Calculate the pH and pOH of the solution at equivalence point pH =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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

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2. Sodium hydroxide absorbs carbon dioxide from the atmosphere, which changes its concentration. In order to verify the exact concentration of NaOH that you make, you will need to standardize it. This is done by performing an acid-base neutralization titration. You will use potassium hydrogen phthalate (KHP) as your acid titrant. Use the steps below to calculate how you will make a KHP titrant. a. How many moles of NaOH would you find in 20 mL of your 0.1 M solution? b. The neutralization reaction between KHP and NaOH shown below. Using stoichiometry, how many moles of KHP would you need to neutralize the moles of NaOH in 20 mL (your answer in part 2a)? NaOH (aq) + KHP (aq) → H2O (1) + NaKP (aq) С. KHP has a molecular mass of 204.43 g/mol. How many grams does your answer in part 2b weigh? d. Take your answer in part 2c and multiply it by two. To make your solution for lab, you will dissolve that much KHP into 100 mL of distilled water. What will the molarity of your KHP solution be?
QUESTION 10 Which of the following is TRUE? OA. An indicator is not pH sensitive. OB. The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. OC. At the equivalence point, the pH is always 7. OD. A titration curve is a plot of pH vs. the [base]/[acid] ratio.
A 5.36–g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L. a. What is the pH of this buffer solution? b. Is the solution acidic or basic? c. What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH . Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL b. 50.0 mL c.100.0 mL d.150.0 mL e. 200.0 mL f. 250.0 mL
120. A diprotic acid with a molar mass of 118.04 g/mol was titrated with 1.023 M NaOH. The equivalence point of the titration occurred at 22.16 mL. Calculate the mass of the acid.
a. Prepare a titration curve for this titration using a graph sheet b. Identify the volume of titrant required to reach the equivalence point of the titration. c. What are the pH, [H30^+], and [OH-] when 21.50 mL of titrant has been added?
49. A 25.00-mL sample of an H₂SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the un- known H₂SO4 solution?
74. A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence point, 40 mL, 50 mL. Sketch the titration curve.
answer and explain step by step
1 If you titrate 25.00 mL of 0.05 M NaOH with 0.025 M HCl, a.what is the hydronium ion concentration at the initial stage with no HCl added yet? b.What is the pH of the solution at the start? c. What is the pH of the solution if you add 25 mL of HCl?
During a titration of HCl and NaOH solution, which chemical substance at the equivalence point determines the pH? a. A buffer forms at this moment in the titration b. Water (H20) with a neutral salt c. OH - from NaOH d. H30 + from HCl
4) A buffer solution is made from 135 mL of 0.395 M in HC2H3O2 and 115 mL 0.345 M NaC2H3O2 (the Ka of acetic acid is 1.79 x 10-5). a. Determine the pH of the initial buffer solution. b. What is the buffering range of this solution? c. What is the buffering capacity of this solution? d. What is the maximum volume of 2.00 M HCl solution you can add this buffer before it is no longer effective?