Question 20 of 25SubmitIn a titration of 21.0 mL of a 0.250M solution of a triprotic acid H3PO4(phosphoric acid) with 0.600 MCa(OH)2, how many mL of base arerequired to reach the thirdequivalence point?mL123C79.+/-x 10 0LO00

Answered: In a titration of 21.0 mL of a 0.25 M…

In a titration of 21.0 mL of a 0.25 M solution of a triprotic acid H3P (phosphoric acid) with 0.600 M Ca(OH)2, how many mL of base required to reach the third equivalence point?

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...

See similar textbooks

Related questions

Q: What volume (in mLmL) of 0.200 M NaOHM NaOH do we need to titrate 36.00 mLmL of 0.140 M HBrM HBr…

Q: In a titration of 47.0 mL of a 0.750 M solution of a triprotic acid H3C6H5O7 (citric acid) with…

Q: In a titration of 18.0 mL of a .250 M solution of a triprotic acid H3PO4 (phosphoric acid) with .800…

Q: 24.0 mL of 0.390 mol/L acetic acid (CH3COOH) is titrated with 0.330 mol/L KOH solution. Calculate…

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

Q: A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH for neutralization to a…

A: Answer: To find out the molar mass of unknown acid it is being titrated against certain quantity of…

Q: 40 mL of NaOH solution with unknown concentration is titrated with 0.10 M of CH3COOH solution in the…

A: From the given data we haveVolume of NaOH (V1)=40mlMolarity of NaOH (M1)=?Volume of…

Q: Suppose a 0.100 M acetic acid is titrated with 0.100 M barium hydroxide. Which of the following…

A: Acetic acid is a weak acid and barium hydroxide is a base. So, it is a acid-base reaction. It is…

Q: In a titration of 14.0 mL of a 0.425 M solution of a diprotic acid H2C4H4O6 (tartaric acid) with…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 10¯1º)

A: The given data contains, pH = 10. Ka=4.9×10-10

Q: What two components must be added to water in order to make a buffer? How would you make an…

A: A buffer solution is a solution whose pH does not change by adding small amount of acid and base.

Q: A solution of 0.600 g of diprotic acid in 100.0 mL of water was titrated with 0.300 M NaOH to the…

A: Solution: Balanced neutralization reaction between diprotic acid and NaOH consider H2A is diprotic…

Q: Consider the following reaction: CH3 COOH + OH- -----> CH3COO- + H2O How much 5.90M NaOH must be…

Q: Assume that 32.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a…

A: Acid and base react with each other to form salt and water. The nature of salt depends on the nature…

Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and…

A: Let y mL benzoic acid and (100 – y) mL sodium benzoate are mixed. For acidic buffer solution, pH =…

Q: What is the pH (in two decimal places) of a weak base-strong acid titration when 25.0 mL of 0.56 M…

A: Volume of NaOCl = 25.0 mlMolarity of NaOCl = 0.56 MVolume of HCl = 23.0 mlMolarity of HCl = 0.34 MKa…

Q: In a titration of 28.0 mL of a 0.425 M solution of a diprotic acid H₂C₄H₄O₆ (tartaric acid) with…

A: The objective of this question is to calculate the volume of base (LiOH) required to reach the first…

Q: In a titration of 80.0 mL of a 0.500 M solution of the diprotic acid H₂C3H₂O4 (malonic acid) with…

A: The balanced equation for the titration is H2C3H2O4(aq) + 2NaOH →Na2C3H2O4 (aq)+2 H2O(l)

Q: How many grams of NaOH must be added to 1.50 L of a 0.400 M solution of oxoacetic acid (HCOCO2H) to…

Q: Calculate the concentration of an HCI solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M…

A: Here we are to required to find the concentration of HCl solution.

Q: In a titration of 16.0 mL of a .425 M solution of a diprotic acid H2C4H4O6 (tartaric acid) with .155…

A: Tartaric acid (H2C4H4O6) is a diprotic acid, which means it can donate two protons (H+) per…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

Q: What is the pH of a weak base-strong acid titration when 20.0 mL of 0.56 M of NaOCl (Ka = 3.0*10-8)…

Q: Consider the following reaction: CH3 COOH + OH- -----> CH3COO- + H2O How much 5.90M NaOH must be…

A: CH3 COOH + OH- -----> CH3COO- + H2O

Q: Calculate the pH at the equivalence point for the titration of 0.170 M methylamine (CH3NH2) with…

Q: 16.17 Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl buffer. What is the pH of the buffer after the…

Q: You are making 100 mL of a 0.44M phosphoric acid buffer with a pH of 7.5. What is the concentration…

A: Given data:Concentration of phosphoric acid buffer = 0.44 MpH = 7.5pKa of phosphoric acid= 2.16

Q: 1. A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.150 M NaOH,…

A: (1) We know that, at equivalence point No. of moles of acid = No. of moles of base No of millimoles…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.90 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: The objective of this question is to find the ratio of sodium cyanide (NaCN) to hydrogen cyanide…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.80 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: Given data is as follows: The pH of the buffer solution = 9.80 The Ka of HCN = 4.9×10-10 The ratio…

Q: Assume that you prepare a buffer by mixing 37 ml of 0.26 M acetic acid and 53 ml of 0.15 M sodium…

A: We have to calculate pH of the buffer solution

Q: In a titration of 38.0 mL of a 0.500 M solution of a diprotic acid H₂C3H₂O4 (malonic acid) with…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.50 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

A: The objective of this question is to find the ratio of sodium cyanide (NaCN) to hydrogen cyanide…

Q: Calculate the mass of ammonium chloride that must be added to 500.0 mL of 0.52 M NH3 to prepare a pH…

A: 1- First calculate the Molarity of ammonium chloride : We will used the Henderson equation, pOH =…

Q: A 4.50-g quantity of a diprotic acid was dissolved in water and made up to exactly 225 mL. Calculate…

A: Given : Mass of acid = 4.50 g Volume of solution made = 225 mL = 0.225 L…

Q: In a titration of 75.0 mL of a 0.500 M solution of a diprotic acid H,C H,O, (malonic acid) with…

Q: In a titration of 68.0 mL of a 0.750 M solution of a triprotic acid H₃C₆H₅O₇ (citric acid) with…

A: Given that - Volume of triprotic acid, citric acid , H₃C₆H₅O₇ = 68.0 mL Molarity of citric acid,…

Q: A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point.…

Q: Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a sample for a…

A: The question is based on the concept of pH of the solution. It is defined as a negative logarithm…

Q: solution

A: Diprotic acid have two equivalence point because it's have two acidic Hydrogens but we need to used…

Q: In a titration of 35.0 mL of a 0.500 M solution of the diprotic acid H₂C₃H₂O₄ (malonic acid) with…

Q: In a titration of 34.0 mL of a 0.250 M solution of a triprotic acid H3PO4 (phosphoric acid) with…

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

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

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

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

Calculate the pH at the equivalence point for the titration of 0.140 M methylamine (CH3NH2) with 0.140 M HCl. The ?b of methylamine is 5.0×10−4.
A 6.25−g quantity of a diprotic acid was dissolved in water and made up to exactly 275 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 11.9 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid were titrated. g/mol
What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 1010)
You have 0.100 M solutions of acetic acid ( p?a = 4.76 ) and sodium acetate. If you wanted to prepare 1.00 L of 0.100 M acetate buffer of pH 4.00 , how many milliliters of acetic acid and sodium acetate would you add?
Bewis a titra on curve of a weak acid with NaOH. What region of the titration curve can the volume of NaOH at equivalence point be located? O с B A 2 A B Vol. NaOH (mL) 6 C 8 10
Calculate the pH at the equivalence point for the titration of 0.190 M methylamine (CH3NH2) with 0.190 M HCl. The ?b of methylamine is 5.0×10−4 M.
A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.150 M NaOH, requiring 16.00 mL to reach the equivalence point. During the titration, the pH after adding 4.00 mL NaOH was 6.912. Calculate Ka for the weak acid.
How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.40? (Ka for HF is 6.8 × 10⁻⁴)
Consider the titration curve for a diprotic acid: 12 10 8 pH 6 4+ 2 + + 10 20 30 Volume of NaOH added (mL) Label the curve with the following items: first equivalence point, second equivalence point, first halfway point, halfway between first and second equivalence points. Determine K, and K, for this diprotic acid. al a2
How many milliliters of 1.50 M NaOH must be added to 2.50×102 mL of 0.12 M NaH2PO4 to make a buffer solution with a pH of 7.00?
O ACIDS AND BASES Calculating the pH of a weak base titrated with a strong acid with a 0.3000 M solution of HNO,. The p K, of An analytical chemist is titrating 160.2 mL of a 0.5000 M solution of dimethylamine ((CH₂)2NH) w dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 280.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places... PH-0 X