The phthalic acid is a diprotic acid (pKa1-2.95, pK₂2-5.41). A titration sample was prepared by dissolving 2.23 g of C6H4(CO₂H)2 in enough water to make 0.120 L. The solution was titrated with 1.552 M NaOH. Calculate the pH at the following points: 1. Before the titration. i eTextbook and Media 2. The 1st midpoint. i 3. The 1st stoichiometric point.

The phthalic acid is a diprotic acid (pKa1-2.95, pK₂2-5.41). A titration sample was prepared by dissolving 2.23 g of C6H4(CO₂H)2 in enough water to make 0.120 L. The solution was titrated with 1.552 M NaOH. Calculate the pH at the following points: 1. Before the titration. i eTextbook and Media 2. The 1st midpoint. i 3. The 1st stoichiometric 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: A 3.81 g sample of alanine (C3H7NO₂), Kb = 7.4 x 10-5) was dissolved in 50.0 cm3 of water.…

A: Given that concentration of HCl = 0.500 M Mass of alanine = 3.81 g Molar mass of alanine…

Q: If the pKa of the indicator is approximately 6, to which of the following equivalence point will it…

A: A suitable indicator should have pH of color transition is given by the equation of pH.…

Q: 1,2-diaminoethane, H₂N-CH₂-CH₂-NH2, is used extensively in the synthesis of compounds containing…

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

Q: Calculate the pH at 25 °C of a 0.80 M solution of potassium butanoate (KC, H,CO,). Note that…

A: Given, [KC3H7CO2] = C = 0.80 M pKa value of HC3H7CO2 = 4.82 Calculate the pH = ?

Q: 11.) Calculate the pH of the following solutions: a.) 0.100 M solution of HNO2 (Ka = 4.5 x 10–4)…

A: (11a)

Q: A 11 mM solution of a compound with a pKa = 6.5(1L total) has a pH of 7.5.If a biochemist adds 9…

Q: Phosphorous acid, H₂PO₂ (aq), is a diprotic oxyacid that is an important compound in industry and…

Q: 1. how many moles of KCN, are required to prepare 250.0mL of a solution with a pOH equal to 2.86

A: 1) pH of a salt formed from weak acid and strong base is pH = 7 + 1/2 ( pKa + log C ) pKa = - log Ka…

Q: Calculate the pH at the second stoichiometric point when 425 mL of 0.046 M solution of tartaric acid…

Q: 5) A 250.0 mL sample of 0.350 M acetic acid (Ka = 1.78 x 10-5) reacted with 2.250 L of gaseous NH3…

A: a) pH = pKa + log([A-]/[HA]) where [A-] is the concentration of the conjugate base, [HA] is the…

Q: 1.Calculate the pH of 0.134 M Sr(OH )2 2. A given weak acid has a pK 3 of 8.18. Calculate the…

A: 1.Calculate the pH of 0.134 M Sr(OH )2 2. A given weak acid has a pK 3 of 8.18. Calculate the…

Q: A chemist titrates 160.0 mL of a 0.6635 M ethylamine (C₂H5NH₂) solution with 0.6870M HNO3 solution…

Q: Let H2A represent a diprotic acid and let A² represent its corresponding base. A 40.0 mL sample of…

A: Diprotic acid is an acid that can give two hydrogen ions (H+) or protons per molecule in an aqueous…

Q: When 50.0 ml of 0.200 M HF(aq) (Ka = 7.0 x 104) is titrated with 20.0 mL of 0.250 M KOH solution.…

A: pKa = -log Ka = - log ( 7 x 10-4) = 4 - log 7 = 4 - 0.85 = 3.15 Millimoles of HF = M x V = 0.200 x…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: Let H2A represent a diprotic acid and let A2 represent its corresponding base. A 40.0 mL sample of…

A: Diprotic acid is an acid that can give two hydrogen ions (H+) or protons per molecule in an aqueous…

Q: A chemist titrates 160.0 mL of a 0.3272M nitrous acid (HNO₂) solution with 0.3027M KOH solution at…

A: In this chemistry problem, we are tasked with calculating the pH at the equivalence point of a…

Q: A buffer solution is prepared by taking 0.250 moles of acetic acid (pK₁ = 4.76) and 0.400 moles of…

A: Number of moles of acetic acid = 0.250 mol Number of moles of barium acetate = 0.400 mol pKa fir…

Q: As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium…

A: To find: How much 1.00 M KH2PO4 will you need to make this solution?

Q: What is the pH of a 0.50 M weak acid solution. The pKa of the weak acid is 11.5. Report 2…

Q: 1. What is the ph of pure water in equilibrium with 1 atmosphere of carbon dioxide at 25 C? 2. What…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: When titrating 225 mL of 0.245 mol/L nitric acid HNO3 with 0.205 mol/L KOH. What is the pH of the…

Q: If 26.7 mL of 0.106 M acid with a pK₂ of 5.37 is titrated with 0.102 M NaOH solution, what is the pH…

A: Please find your solution below : Acid-base titration is a method of qualitative analysis in which…

Q: Calculate the pH of a buffer solution containing 0.58 moles of sodium acetate (NaC2H3O2) and 0.43…

A: The detailed explanation is provided below.

Q: 4. A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium…

Q: If 40.0 mL of formic acid with a concentration of 0.300 M and a Ka of (2.258x10^-5) is titrated with…

Q: None

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

The phthalic acid is a diprotic acid (pKa1-2.95, pKa2-5.41). A titration sample was prepared by dissolving 2.23 g of C6H4(CO2H)2 in
enough water to make 0.120 L. The solution was titrated with 1.552 M NaOH. Calculate the pH at the following points:
1. Before the titration.
i
eTextbook and Media
2. The 1st midpoint.
i
3. The 1st stoichiometric point.
i

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

Step 2

Step 3

Step 4

Step by step

Solved in 4 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

What is the resulting pH if 2.0 mL of a 100 mM HCl solution is added to 100 mL of a 10.0 mM solutionof phosphoric acid at pH = 7.0? (The pKa values of phosphoric acid are 2.1, 7.2, and 12.3.)
A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)
Reaction: NaHCO3(aq) + HCl(aq) ® NaCl(aq) + CO2(g) + H2O(l) Methyl orange is a pH indicator. It is yellow above pH 4.4, orange between pH 4.4 and 3.2 and red below pH 3.2. NaHCO3 is a weak base and it must be acidified to about pH 4 to completely neutralize it. Why did you test the reaction mixture with this indicator before you began the evaporation step?
What is the pKa of an unknown monoprotic acid solution of 0.0450 M at pH 2.78
ch2
A 100 mL buffer solution that is pH 8.06 buffer is prepared by first adding 0.45 grams of RNH2 (121.1 g/mole) into a beaker. To make the solution, how many mL of a stock solution of 1.0 M R-NH3+ solution should be added to the beaker before diluting to 100 mL?
Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06. (pKa = 4.76) 0.3:1 1.99:1 0.50:1 1.51:1 What is the correct answer? 1,2,3 or 4?
23. A 1 L solution initially contained 0.42 M fluoride anion and 0.33 M HF (K₂ = 7.2 ×10¯4). What is the pH of the solution described if the following additions are made: a. 100 mL of 0.2 M HCl (added to original solution): b. 100 mL of 0.2 M NaOH (added to original solution): A: 3.20; 3.29
#5
A titration of 35.0 mL of an unknown tribasic salt, Li₃A, requires 90.00 mL of 0.250 M HCl to reach the 3rd equivalence point. The titration data is shown below: Vol of HCl (mL) 15.00 30.00 45.00 60.00 75.00 90.00 pH 10.45 8.62 6.79 4.86 2.93 1.35 What is the value of Kb₁ of A³⁻?
A group of students perform a titration experiment. The buret tube is filled to the 0.00ml line with 0.100M NaOH solution. The E. flask contains 50.0ml ov 0.100M HC2H3O2 solution. The Ka of the acetic acid is: Ka = 1.8 x 10-5. A) Write the ionic equation for the conjugate acid reactihng with water. One product is the OH- polyatomic ion. B) What is the pH of the equivalence point?
An aqueous solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka= 6.3 × 10-5for HC7H5O2. Thesolution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?