Answered: Calculate the pH at the equivalence…

Calculate the pH at the equivalence point for the titration of 0.220 M methylamine (CH3NH2) with 0.220 M HCl. The Kb of methylamine is 5.0×10−4.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.42QAP

See similar textbooks

Related questions

Q: Describe acid-base titration. What is the equivalence point?

A: Titration is one of the most common method of qualitative analysis of substances given. It is done…

Q: 5.)20.0 ml of 0.200M hypobromous acid, HBrO, is titrated with 0.250M sodium hydroxide, NaOH.…

A: Volume of HBrO = 20 mL Molarity of HBrO = 0.200 M Molarity of NaOH = 0.250 M To determine pH at…

Q: What is the pH at the equivalence point if it requires 28.50 mL of 0.1208 M KOH to completely…

A: Solution- Introduction According to Le Chatelier’s principle, “When a system experiences any…

Q: Calculate the pH at the equivalence point for titrating0.200 M solutions of each of the following…

A: (a) Given, The concentration of NaOH solution is 0.200 M The concentration of HBr solution is 0.200…

Q: At the equivalence point in the titration of 0.260 M CH3NH2(aq) with 0.260 M HCl(aq), why is the pH…

A: Given, At the equivalence point in the titration of 0.260 M CH3NH2(aq) with 0.260 M HCl(aq), the pH…

Q: Describe the process of calculating a weak acid–strong base Titration?

A: Titration: Titration is quantitative analysis where concentration and amount of unknown sample is…

Q: When titrating a weak acid with a strong base, it is found that the equivalence point happens when…

A: equivalence point of any acid base titration is that point where equal no of moles of both the…

Q: Calculate the pH and the concentrations of all species halfway to the first equivalent point in the…

A: pH is the measure of acidity of a solution. It is defined as negative logarithm (to base 10) of…

Q: Define equivalence point, and describe the steps involved in determining it for weak acid-strong…

A: It is the point at which the amount of base added has completely neutralized the acid solution.At…

Q: Calculate the pH in the titration of 25.0 mL of 0.100 M acetic acid by sodium hydroxide after the…

A: Given volume of acetic acid is 25.0mL and strength is 0.100 M. Given volume of NaOH is 30.0 mL and…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (Ka of HCN is 4.9 x 10 10)

Q: Which of the following titrations is the MOST feasible? HI versus KOH NH4CI versus HCI acetic acid…

Q: Calculate the pH value when titrated between 25 ml of weak acid HA concentration of 0.3 (104 x 6.6…

Q: d. In another experiment, the student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH.…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: A solution is formed by adding 3.20 grams of solid sodium hypochlorite, NaClO, to 500.0 ml of…

A: Answer: Solution will be basic due to hydrolysis of hypochlorite ion because it is the conjugate…

Q: If equal volumes of 0.29 M acetic acid and 0.12 M sodium hydroxide are mixed, what is the pH of the…

A: Henderson–Hasselbalch equation, pH = pKa + log [salt]/[acid]

Q: A sample containing 50.00 mL of 0.1000 M hydrazoic acid (HN3) is being titrated with 0.1000 M sodium…

Q: Calculate the pH for each of the cases in the titration of 35.0 mL of 0.200 M NaOH(aq) with 0.200 M…

Q: In an experiment, a student titrated 50.0mL of 0.100M HC2H3O2 with 0.100M NaOH(aq). Calculate the pH…

A: Volume= 50.0 mL Concentration of HC2H3O2( CH3COOH)=0.100M Concentration of NaOH=0.100M pH of the…

Q: Calculate the pH at the equivalence point in titrating 0.100M solutions of each of the following…

A: The point in the titration in which the analyte is completely neutralized by the titrant that is the…

Q: the titration of 0.100M acetic acid with 0.100M NaOH is described in the text. wha

A: Given volume of acid(acetic acid) = 0.100L Concentration of acid(acetic acid) = 0.100M Volume of…

Q: 4. Define equivalent point and end point in a titration between a strong acid and strong base.

A: Strong acid : In aqueous solution they undergoes complete dissociation to form H+ ion and the…

Q: Calculate the pH at the equivalence point for these titrations: a) 0.10M HCl with 0.10M NH3. b)…

Q: calculate the pH at the equivalence point for the following titration: 0.20M HCL versus 0.20M…

A: Ka= Kw/Kb CH3NH2 +HCl ------>CH3NH3+ + Cl-

Q: You are running a titration. You have placed 40.0 mL of 0.200 M chlorous acid, HCIO2, in a flask and…

A: mmoles of HClO2 = 40 x 0.2 = 8 mmoles mmoles of KOH = 80 x 0.1 = 8 mmoles KOH + HClO2 ----->…

Q: Calculate the pH of a buffer solution that is 2.00 M in phosphoric acid and 1.50 M in potassium…

Q: Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following…

A: It is given that 0.080 M NaOH is reacting with the given 0.100 M solutions and to calculate the pH…

Q: How does the titration curve of a monoprotic acid differ from that of a diprotic acid?

A: In chemistry, there are many ways to check the deviation of experimental data from the accurate…

Q: The pH of 300 mL solution made of 0.93 M acetic acid and 1.07 M potassium acetate is (K, = 1.8 x…

Q: A solution of the weak acid HA is prepared by dissolving 2.20 g of HA in 100.0 mL water. The…

A: Given: Mass of HA = 2.20 g. Concentration of NaOH = 0.500 M Volume of NaOH solution required = 31.1…

Q: pH

Q: Calculate the pH at the stoichiometric point when 25 mL of 0.10 M pyridine is titrated with 0.32 M…

A: Moles can be calculated by using following formula,Moles = Molarity × Volume

Q: 15. A 25.0 mL solution of 0.250 mol/L methanoic acid, HCOOH(aq), is titrated with a 0.100 mol/L…

Q: Consider the titration of 90.0 mL of .141 M Ba(OH)2 by .564 M HCl. Calculate the pH of the resulting…

A: In the given question we have to calculate the pH of Solution after adding acid of 11.0 mL and 27.0…

Q: Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.

A: The Henderson hasselbalch equation for calculation of pH of a buffer is pH = pKa + log[base][acid]…

Q: What volume of base is required to reach the equivalence point in a titration of 20.00 mL of 0.11 M…

Q: If 27.9 mL of 0.200 M NaOH was required to reach the equivalence point in the titration of 100 mL of…

A: The question is based on the concept of titrations. we are titrating a weak acid with a strong…

Q: Describe the pH changes that occur during the titration of a weak base by a strong acid. What is…

A: A reaction between a base and an acid to give water and salt as products is known as the…

Q: What is the difference between endpoint and equivalence point in acid-base titration?

Q: Write the titration reaction of 100 mL of 0.100 M anilinium bromide (“aminobenzene . HBr”) +.100 M…

A: In analytical chemistry, titrations are carried out to determine the concentrations of unknown acids…

Q: Calculate the pH for each case in the titration of 50.0 mL of 0.120 M HCIO(aq) with 0.120 M KOH(aq).…

A: Note - Since you have asked a question with multiple subparts, we will do the first three subparts…

Q: 1 Calculate the pH and the concentration of all species at the start of the titration of 0.100 M…

A: An acid is a chemical species that can enhance the concentration of H+ ions in an aqueous solution.…

Q: For the titration of 10 mL of 0.15 M acetic acid with 0.1 M sodium hydroxide, what is the pH when…

Q: In the titration of a 25.00 mL sample of the hypothetical monoprotic acid, CHEM, it took 20.41 mL of…

Q: It is titrated with 50 mL of 0.025M NH3 and 23 mL of 0.05M HCI. Calculate the pH value of the…

A: In this question, we have to find out the correct answer of given problem by the help of THE…

Q: Titrations: Calculate the pH when 73 mL of 1.25 M ammonia (K = 1.8x10-) is added to 28 mL of 0.85 M…

A: 1.) To calculate pH , first we would Calculate moles of both acid and base. Then we would write a…

Q: Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following…

A: Given: Concentration of NaOH= 0.080M To find: The pH at the equivalence point

Q: Calculate the pH in the titration of 25 mL of 0.10 M HCl by sodium hydroxide after the addition to…

A: Welcome to bartleby !

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%

Calculate the pH at the equivalence point for the titration of 0.220 M methylamine (CH3NH2) with 0.220 M HCl. The Kb of methylamine is 5.0×10−4.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps with 6 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

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.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of (a) NaOH with HClO4. (b) acetic acid with KOH. (c) NH3 solution with HBr. (d) KOH with HNO3. Explain your choices.
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Chloropropionic acid, ClCH2CH2COOH, is a weak monoprotic acid with Ka = 7.94 105. Calculate the pH at the equivalence point in a titration of 10.00 mL of 0.100 M chloropropionic acid with 0.100 M KOH. Choose an indicator from Table 16.4 for the titration. Explain your choice. TABLE 16.5 Properties of Several Indicators
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
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?