A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 mL Added, pH = Part 2 of 4 10.0 mL Added, pH = I 0 10 X

A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K, of bases at 25 °C tables for additional information. Part 1 of 4 0.00 mL Added, pH = Part 2 of 4 10.0 mL Added, pH = I 0 10 X

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.3QE: Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify...

See similar textbooks

Related questions

Q: An analytical chemist is titrating 141.2 mL of a 0.4100M solution of piperidine (C,H1,NH) with a…

Q: Which of the following acid and base species, when mixed together in a 1:1 mole ratio, will make a…

A: From the given following options, which will give buffer solution when mixed together in 1:1 mole…

Q: During the titration, how would your experimental molarity of NaOH differ from the actual molarity…

A: Please have a look on the solution:

Q: 3. a. Find the pH of a solution that is 0.25 M NH, and 0.10 M NH.CI given that the K. for NH" is…

Q: 1. Value of pKal from graph. 25 2. Value of pKa2 from graph. 3. Value of Kal- 4. Value of Ka2. Using…

A: A polyprotic acid is a weak acid that contains more than one ionizable protons in its most…

Q: Calculate the [OH-] and pH of a mixture formed by adding 50.0 mL of 0.0.20 M HCl to 150 mL of 0.010…

A: Given : Concentration of HCl = 0.020 M (Assuming…

Q: A solution made by mixing 125.00 mL of 0.950 M HOCI with 50.00 mL of 0.800 M NaOH. How can I find…

A: The objective of this question is to find the pH of a solution made by mixing 125.00 mL of 0.950 M…

Q: Adding 100. ml of 0.120 M HCl to 200. ml of 0.200 M NH3, calculate the pH for the solution (pKb=…

Q: What is the pH of a solution made by mixing 24.0 of NaF and milling it up making 500 mL of solution?…

Q: 2. Consider a 200.0 mL solution that is 0.00155 M in HCl and 0.0200 M in HCIO2 ww a) Calculate the…

A: The pH of a solution is used to determine the alkalinity or acidity of a solution. The pH is simply…

Q: 8. A 1.000 L buffer solution contains 0.250 mol/L. NH, and 0.250 mol/L. NH, CL K=1.8x10 Determine…

A: We have to calculate the pH

Q: .100 moles of HCI is added to a 1L mixture of .100M HC3H5O2 and 0.180M KC3H5O₂. Assuming no volume…

Q: Let X represent a nonmetal. Which of the following buffer solutions functions at the lowest pH? More…

A: pH of a buffer consisting of a weak acid and salt of same acid with a strong base can be calculated…

Q: 1. A student uses a solution of 0.30 mol/L HCI to titrate a 45.0 mL solution of 0.35 mol/L…

A: The objective of the question is to find the pH of the solution.Given data:The molarity of…

Q: A 11.5 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCI. What is the pH of the…

A: pH of solution is 12.71 Explanation:Step 1: To find the pH of the solution after adding 2.77 mL of…

Q: 335 mL of a 0.47 M hydroiodic acid solution is added to 388 mL of a 0.36 M perchloric acid solution.…

A: PH = -log[H+] PH + POH =14

Q: S.No SOLUTION H* OH- pH РОН 1 0.15 М НI 2 0.040M KOH 3 0.020M Ва(ОН). 4 0.00030M ----- -- HCIO, 5…

A: As you not specified so i am giving first 3 answers as per guidlines Use the relation Ph=-log(H+)…

Q: 2. For each of the following salts, determine the pH of a 2.50M solution of the salt. You will need…

A: Molar concentration of solution of salt = 2.50 M

Q: The [H+] = 1.1 x 10-3 M for the NaF / HF solution in the previous step. What is the pH of the…

Q: 5. Show the full calculations necessary in order to calculate the pH of the resulting solution after…

Q: 16. A 100.0 mL solution of 0.15 M acetic acid is tiated sing 0.20 M potassile hydroxide. Let's…

A: The objective of this question is to calculate the pH at the endpoint of a titration between acetic…

Q: A 10.0 mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate the pH after…

A: First, we need to calculate the initial moles of NH3. The number of moles is given by the formula:n…

Q: A 17.8 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What is the pH of the…

Q: A 17.2 mL solution of 0.100 mol L-¹ HF is titrated using 0.150 mol L-1 NaOH. What is the pH of the…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: 4. If you titrate 100 mL of an unknown strong acid solution with 0.1 M NaOH, will the pH ever reach…

A: Acid base titration: In acid base titration a solution of known concentration is added to a…

Q: A 150.0 mL sample of 0.21 M HF is titrated with 0.50 M NaOH. Determine the pH at these points: At…

Q: In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100…

Q: Please don't provide handwritten solution...

A: Solution: Determine Concentration of Pyridine at Equivalence Point: At the equivalence point of the…

Q: A 10.0 mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate the pH after…

A: First, we need to calculate the initial moles of NH3. The number of moles is given by the formula: n…

Q: A 10.0 ml solution of 0.330 M NH, is titrated with a 0.110 M HC1 solution. Calculate the pil after…

Q: Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

100%

35
A 10.0 mL solution of 0.330 M NH3 is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL,
10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places.
Note: Reference the K of acids at 25 °C and K² of bases at 25 °C tables for additional information.
a
Part 1 of 4
0.00 mL Added, pH =
Part 2 of 4
10.0 mL Added, pH =
x10
X
x10
X

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: 0.00 mL added

VIEW

Step 2: 10.0 mL added

VIEW

Step 3: 30.0 mL added

VIEW

Step 4: 40.0 mL added

VIEW

Solution

VIEW

Step by step

Solved in 5 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
The pH of 0.10 M CH3NH2 (methylamine) is 11.8. When the chloride salt of methylamine, CH3NH3Cl, is added to this solution, does the pH increase or decrease? Explain, using Le Chteliers principle and the common-ion effect.
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.
Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the major species in solution at equilibrium (besides water), and what are their concentrations?
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?
Calculate the mass in grams of ammonium chloride, NH4C1, that would have to be added to 500. mL of 0.10-M NH3 solution to have a pH of 9.00.
A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?
Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
Which of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.