The Ka of formic acid HCOOH is 1.77 x 10. A 0.60 M formic acid solution of 40.0 mL is titrated with 0.40 M NaOH. Which of the following statements is correct regarding the above titration?O a. After adding 60.0 ml of NaOH, the pH of the resulting solution is greater than 7.O b. After adding 20.0 ml of NaOH, the pH of the resulting solution is calculated as pH = pka.OC. After adding 40.0 mL of NaOH the pH of the resulting solution is greater than 7.The pH of 0.60 M of formic acid solution of 40.0 mL is greater than 7.Od.O e. After adding 30. 0 ml of NaOH, the pH of the resulting solution is equal to the pkp of format ion (HCOO").

Mmol of formic acid = M × V = 0.60 × 40 = 24 mmol After adding 60 mL of NaOH, Mmol of NaOH =…

Answered: 3 60.0 ml of NaOH, the pH of the…

3 60.0 ml of NaOH, the pH of the resulting solution is greater than 7. g 20.0 mL of NaOH, the pH of the resulting solution is calculated as nH nka

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: HF is a weak acid and NH3 is a weak base. Which of the following shows the correct order of…

A: Sodium chloride is formed from the reaction of a strong acid and a strong base. In the formation of…

Q: A 25.0 mL volume of a sodium hydroxide solution requires 19.6 mL of a 0.189 M HCl solution for…

A: The objective of this question is to calculate the concentration of the phosphoric acid solution…

Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: Answer:- Henderson-Hasselbach equation :- This equation is used for the determination of pH or pOH…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

Q: What volume of 0.100 M acetic acid is needed to reach the equivalence point with 25.00 mL of 0.200 M…

A: One mole of acetic acid reacts with one mole of sodium hydroxide to form one mole of sodium acetate…

Q: A solution is composed of 30 mL of 2.5 M H2SO4 and 25 mL of 6.4 N KOH. The resulting solution is…

Q: calculate the ph of the following solutions a 0.15M KNO 2 b 0.34 M NaOCI c. 0.28 M NH4Br

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00577 M HCIO4 pH = (b) 0.523…

A: a) pH of a solution of 0.00577 M HClO4 (perchloric acid)pH=−log [H+]In the case of a strong acid…

Q: Calcium bydroxide may be used to neutralize (completely react with) aqueous hydrochlcric acid.…

A: The balanced reaction will look like, 2HCl + Ca(OH)2 → CaCl2 + 2H2O It is given that,amount of solid…

Q: Which of the following solutions will have the lowest pH value? A.) 0.10 M HNO3 B.) 0.03 M H2SO4…

A: Given acids: A.) 0.10 M HNO3 B.) 0.03 M H2SO4 C.) 1.0 M HCN (Ka = 4 X 10-10) D.) 2.0 M…

Q: A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

Q: 7a Calculate the pH of a solution if its [H;O*] is 5.5 x 106 7b Calculate the [OH] of a solution…

Q: A solution is prepared by adding 50.0 mL concentrated hydrochloric a and 20.0 mL concentrated nitric…

Q: Calculate the pH of a solution, during the titration of 60.2 mL of 0.148 M KOH, after adding 39.9 mL…

A: The reaction between an acid molecule and a base molecule to form an ionic compound along with water…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00704 M HIO4 pH = (b) 0.696 g…

A: The objective of the question is to calculate the pH of different solutions of a strong acid, HIO4.…

Q: i. 200 mL of a 0.200 M solution Disodium phosphate (Na,HPO) to which 60 mL of 1.0 M HCI is added. pH…

A: Answer: pH of a solution is equal to the negative of logarithm of its hydrogen ion concentration.

Q: 300 ml of 0.25M KHPO is added to 30 ml of 0.38 M HCl. Pure water is added to 4 bring the final…

A: Given -> Volume of KH2PO4 = 300 ml = 0.300 L (1L = 1000ml) Molarity of KH2PO4 = 0.25 M Molarity…

Q: In blood plasma, pH is maintained by the carbonic acid-bicarbonate buffer system. How is pH…

A: The equilibrium reaction taking place in body is as follows: When acid is added to the buffer…

Q: students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

Q: When 0.152 mol of a weak acid, HX, is dissolved in 2.00 L of aqueous solution, the pH of the…

Q: In the year 1980, countries near the United States experienced an increase in acid precipi- tation.…

A: The burning of Fossil fuels produces acidic oxide like sulfur dioxide or nitrogen dioxide etc. which…

Q: When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the…

A: Given, Volume of NaOH = 14.08 mL Molarity of NaOH = 0.1594 M Volume of unknown weak acid =25.00 mL…

Q: What is the concentration of the unknown HCl solution in M?

Q: HF is a weak acid and NH3 is a weak base. Which of the following shows the correct order of…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: In a system at equilibrium, the concentration of the NH3(aq) is 0.35 mol/L and the concentration of…

A: Concentration of NH3 = 0.35 MConcentration of NH4Cl = 0.25 MKa value of ammonia = 5.6*10-10pH =?

Q: a) The average pH of normal arterial blood is 7.40 at 37° C. Calculate [H] for blood at this…

A: a) Given : pH of blood = 7.40

Q: A solution containing 2.60 x 10-3 moles of HCl and 3.32 x 10-3 moles of NaOH into a container and…

A: Given:- For a solution in a container, No of moles of HCl = 2.60 x 10-3 No of moles of NaOH = 3.32…

Q: How many mls of 0.125 M HCl must be added to 65.5 mls of 0.234 M NH3 to completely neutralize the…

A: Given, Molarity of HCl solution = 0.125 M = 0.125 mol/L Volume of NH3 solution = 65.5 mL = 0.0655 L…

Q: A chemist makes a 1.0 L of a solution that is both 0.6 M NH, and 0.8 M NH,CI. pK, of NH3 = 4.75.…

A: Given :- Concentration of NH3 solution = 0.6 M Concentration of NH4Cl = 0.8 M Volume = 1 L pKb…

Q: 6) Which of the following has the highest hydroxide ion concentration? 0.1 M HCI 0.1 M H₂SO4 a…

Q: For a titration of 50.0 mL of 0.100 M HCl, what is the pH of the solution when 40.0 mL of 0.100 M…

Q: Suppose that a benzoic acid (C,H,COOH) solution has a pH of 3.15. Which of these substances would…

A: Given substances: KCl C6H5COONa NaI HBr We have to find the substance that would increase the pH…

Q: How much 0.500 M NaOH should be added to 12.0 g of tris hydrochloride to reach pH 7.77 in a final…

A: Given, Molarity of NaOH = 0.5 MAmount of tris-hydrochloride (T-HCl) = 12 gFinal pH = 7.77Final…

Q: HF is a weak acid and NH3 is a weak base. Which of the following shows the correct order of…

Q: 10 g of the strong base Ba(OH)2 is dissolved in 200 mL of water and then turreted with 0.100 M HCl.…

Q: What is the pH of a solution resulting from 5.00 mL of 0.011 M HCl being added to 50.00 mL of pure…

A: 5.00 mL of 0.011 M HCl solution is diluted with 50.00 mL of pure water.Determine the concentration…

Q: 36. Which will have a lower (the lowest) pH among the solutions shown in each of the following…

A: a) 0.001 M NaOH and 0.005 M NaOH Since NaOH is a strong base hence it will dissociate completely…

Q: A buffer solution is prepared by adding 6.16 mL of 1.37 M HBr to 195.0 mL of 0.14 M NH3. Then, 0.005…

A: Step 1:First we determine the initial moles of HBr and NH₃: For HBr: Moles of…

Q: Sodium hypochlorite solution is also known as bleach. It contains the hypochlorite ion ClO-. (a)…

Q: Calculate the pH change that results when 12 mL of 2.1 M HCl is added to 560. mL of each of the…

A: pH change = pH of final solution - pH of initial solution pH = pHfinal - pHinitial

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

Q: If 50 ml 0.40 M HCl is added onto the 40 ml 0.15 M NaCN solution, what is the final ph?

Q: in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The…

A: The compounds that doesn't dissolves completely are termed as covalent/molecular and weak…

Q: Which has a higher pH? O 0.10 M of a strong acid 0.10 M of a weak acid Neither, both have the same…

A: 37. Strong acids have higher concentration of hydronium ions compared to weak acid. Increase in…

Q: What volume of .155 M of NaOH is required to titrate 18.5 ml of .12 M of HCl

Q: Which of the following sets of compounds, when dissolved in the same solution. forms a buffer…

A: Which of the following sets of compounds, when dissolved in the same solution, forms a buffer…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

The Ka of formic acid HCOOH is 1.77 x 10. A 0.60 M formic acid solution of 40.0 mL is titrated with 0.40 M NaOH. Which of the following statements is correct regarding the above titration?
O a. After adding 60.0 ml of NaOH, the pH of the resulting solution is greater than 7.
O b. After adding 20.0 ml of NaOH, the pH of the resulting solution is calculated as pH = pka.
OC. After adding 40.0 mL of NaOH the pH of the resulting solution is greater than 7.
The pH of 0.60 M of formic acid solution of 40.0 mL is greater than 7.
Od.
O e. After adding 30. 0 ml of NaOH, the pH of the resulting solution is equal to the pkp of format ion (HCOO").

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

VIEW

Step 2

VIEW

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

If 250.0 mL of HNO3 are reacted with 34.8 mL of 0.721 M Ba(OH)2, to reach the equivalence point, what is the pH of the original HNO3 solution?
A student mixes 300 mL of 0.100 M NAOH with 100 mL of 0.300 M H,SO4. The resulting solution has a pH of O 14.000 O 13.800 000
A 39.0 mL sample of a 0.540 M aqueous hypochlorous acid solution is titrated with a 0.390 M aqueous solution of sodium hydroxide. How many milliliters of sodium hydroxide must be added to reach a pH of 7.176? mL
You take a 1.50 moles of strong acid HCl and a 1.00 moles strong base NaCl and combine them with a total volume of 1.00 Liter. What is the pH of the solution? What is the [OH-] of the solution? What is the [Cl-] in the solution? What is the [Na+] in the solution?
Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical speci written in the second column of the table. Use the checkboxes to classify each compound. type of compound (check all that apply) important species present when dissolved in water lonic molecular strong weak strong weak base compound acid acid base C,H,NH, c,H,NH, OH , C,H,NH,, H,0 HC,H,0, H,0", C,H,0,, HC,H,0,, H,0 КОН к", он , н,о H BrO4 H,0", Bro,, H,0
The pH after adding 21.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is 0.087 0.16 0.80 1.1
Calculate the pH of each of the following strong acid solutions. (a) 0.00532 M HCI pH: = (b) 0.794 g of HCIO4 in 33.0 L of solution pH = (c) 48.0 mL of 3.20 M HCl diluted to 3.20 L pH: = (d) a mixture formed by adding 54.0 mL of 0.00540 M HCI to 90.0 mL of 0.00120 M HCIO4 pH = =
How many milliliters of 0.0334 M KOH are needed to completely neutralize the HCI in 430 mL of a hydrochloric acid solution that has a pH of 2.91? mL 0.0334 M KOH
Assume negligible volume change of solution every other addition. 1. Using 12.0 mL 0.25 M CH3COOH-12.0 mL 0.25 M NaCH3COO, find the pH of the solution if we add 0.15 mL of 1.0 M of HCI? 2. Using 12.0 mL 0.25 M CH3COOH - 12.0 mL 0.25 M NaCH3COO, find the pH of the solution if we add 0.15 mL of 1.0 M of NaOH? 3. Using 12.0 mL 0.25 M NH3-15.0 mL 0.20 M NH4CI, find the pH of the solution if we add 0.15 mL of 1.0 M of HCI? 4. Using 12.0 mL 0.25 M NH3 - 15.0 mL 0.20 M NH4CI, find the pH of the solution if we add 0.15 mL of 1.0 M of NaOH?
What mass of Ca(OH) is required to neutralize 50.00 mL of 0.180 M HCI?
10g of the strong base Ba(OH)2 is dissolved in 200 mL of water and then titrated with 0.100 M HCl. How many mL of the acid solution must be added to exactly neutralize the solution?
In a titration experiment, 12.5 mL of 0.500 M H2SO4 neutralizes 50.0 mL of NaOH. What is the concentration of the NaOH solution? When formulating an equation for the aboce problem, how do I know what to combine and why is OH- left out?