What volume of 0.1543 M NaOH must be added to 25.00 mL of 0.2405 M HCOOH in order to prepare a solution of pH=3.7? Explain and justify any simplifying assumptions made in your calculation. KA of HCOOH = 1.8 x 104 M %3D

What volume of 0.1543 M NaOH must be added to 25.00 mL of 0.2405 M HCOOH in order to prepare a solution of pH=3.7? Explain and justify any simplifying assumptions made in your calculation. KA of HCOOH = 1.8 x 104 M %3D

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: Determine the pH of the resulting solution by mixing 0.36 M of sodium formate (HCOONa) of 20.0 mL…

A: As 0.36M of sodium formate of 20.0 ml is mixed with 0.18 M of HCl of 40.0 mL, thus equivalence point…

Q: Calculate the mass of sodium acetate (CH3COONa) required to prepare 35 mL of a 0.15 M sodium acetate…

A: Given data: Sodium acetate concentration = 0.15 M Volume = 35 mL Molar mass of sodium acetate =…

Q: Determine the pH of a solution that is 0.15 M CH3COOH and 0.10 M CH3COONa.

A: Given that Ka for CH3COOH = 1.8 × 10–5 Concentration of CH3COOH = 0.15 M Concentration of CH3COO–…

Q: Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 46.0 mL of 0.400 M CH NH2 (Kb = 4.4 ×…

A: Given: Concentration of HBr = 0.200 MVolume of HBr solution = 45.0 mL = 0.045 L…

Q: 18) How many grams of sodium fluoride (MM =41.988 g/mol) must be added to 250.0 mL of a 0.100 M…

A: This question based on formula of acidic buffer NaF and HF is acidic buffer The answer is c that…

Q: Calculate the pH of the resulting solution when 25.0 mL of 0.30 M HClO4 is added to 60.0 mL of 0.35…

A: Henderson-Hasselbach equation: pH=pKa + log Conjugate baseWeak acidpOH=pKb + log Conjugate acidWeak…

Q: 1.33 mol HF is added to enough 0.434-M NaF solution to give a final volume of 1.7 L. What is the pH…

A: The pH of this buffer solution can be determined by using Handersson hasselbalch equation for weak…

Q: Calculate the pH of the resulting solution when 30.0 mL of 0.16 M KOH are added to 46.0 mL of 0.15 M…

A: When KOH ( a strong base ) is added to HClO ( a weak acid , they would react to form a buffer…

Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…

Q: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.16 M NH3 with 25.00 mL of 6.0 × 102…

A: pKb = - log Kb = - log (1.80 * 10-5 ) = 4.745pKa = 14-pKb = 14- 4.745…

Q: 1) Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COONa, in 78.0…

A: Data

Q: Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H502 with 100.0 mL of 0.30 M…

Q: Suppose 1.00 mol of CgH;COOH and 0.500 mol C,H;COONA are added to water and diluted to 1.00 L. The…

A: a. Benzoic acid and sodium benzoate forms acidic buffer solution. Henderson equation for acidic…

Q: Determine the pH of a solution that is 0.20 M CH3COOH and 0.15 M CH3COONa.

A: Given :The solutions given are 0.20 M CH3COOH and 0.15 M CH3COONa.We need to pH of the solution.

Q: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.20 M NH3 with 25.00 mL of 5.0 x 10-2…

Q: How many moles of BHCl (acidic salt) would need to be added to 437 mL of 1.3 M B (a weak base) to…

A: pH + pOH = 14 pOH = pKb + log[salt]/[base] pKb = -logKb

Q: pH

Q: dont provide handwritiing solution ...

A: The objective of this question is to calculate the pH at the equivalence point of a titration…

Q: How many moles of B (weak base) would need to be added to 507 mL of 0.28 M BHCl (the acidic salt) to…

A: IMPORTANT POINTS: It is the case of basic buffer containing a weak base and its conjugate salt BHCl…

Q: A solution is prepared that is initially 0.41 M in pyridine (C,H,N), a weak base, and 0.20M in…

A: initial changefinal

Q: Sodium bicarbonate gives solutions that are slightly alkaline (approximately pH 8.3), and similar…

A: Here we have to determine the pH of 0.26M Sodium carbonate solution.

Q: 1.0 M HCl solution has a volume of 20.0 mL. Determine the pH of the solution that results from…

A: The balanced chemical equation for the given reaction is,

Q: What is the pH of a solution prepared by mixing exactly 25.0 mL of 0.200 M HC₂H3O2 with 15.0 mL of…

A: Given data The concentration of HC2H3O2 is 0.200 M The volume of HC2H3O2 is 25.0 mL The…

Q: A 1.00 L volume of solution contains 0.250 M HC2H3O2 and 0.240 M NaC2H3O2 at pH 4.72. To the…

A: Since NaOH(aq) is a monoacidic strong base, it reacts with the acidic part, HC2H3O2(aq) of the…

Q: 1). The sample of 25.00 mL of 0.010 M HCOOH is titrated with 0.020 M KOH. (a) Show the reaction…

A: Since you have asked question with multiple subpart, we will solve the first three subpart question…

Q: Determine the pH of the resulting solution by mixing 0.36 M of sodium formate (HCOONA) of 20.0 mL…

Q: ||| O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the…

A: The question is based on the concept of salt hydrolysis. we need to arrange the salts in increasing…

Q: Calculate the pH of a solution formed by adding 8.00 grams of solid sodium azide, NaN3, to 210.0 ml…

A: Molarity of Sodium Azide = 0.230 MVolume of Solution = 210.0 mLamount of sodium azide = 8 gMolar…

Q: A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is bubbled into a 0.400 L solution of…

A: To calculate the pH of the resulting solution after adding ammonia () gas to hydrochloric acid (HCl)…

Q: A chemist titrates 130.0 mL of a 0.7778 M lidocaine (C, H,,NONH) solution with 0.1602 M HCI solution…

A: Given: Concentration of lidocaine, M1= 0.7778 MVolume of lidocaine, V1= 130ml =0.130LConcentration…

Q: Calculate the pH of the solution when 35.0 mL of 0.15 M HCN is mixed with 17.5 mL of 0.30 M NaOH. Ka…

A: [NaOH ] = 0.30 M VNaOH = 17.5 ml nNaOH = 0.30 M x 17.5ml = 5.25 m mol [HCN ] = 0.150 M V HCN =…

Q: calculate the pH of a solution formed by mixing 0.172 L of 1.77 M NH4Cl with 0.5323 L of 2.61 M NH3.…

Q: dont provide handwriitning solution..

A: The objective of this question is to calculate the pH at the equivalence point of a titration…

Q: How many moles of B (weak base) would need to be added to 527 mL of 0.38 M BHCl (the acidic salt) to…

Q: Calculate the pH of the solution when 45.0 mL of 0.25 M HNO2 is mixed with 45.0 mL of 0.35 M NaOH.…

Q: Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 HCOOH with 100.0 mL of 0.20…

A: A mixture of a weak acid (HCOOH in the given case) and its salt with a strong base (HCOOLi in the…

Q: Can you please further explain to me what I have to do to find the theoretical pH? I've prepared a…

A: We know weak acids are not completely dissociated into ions so their pH is mainly determined by some…

Q: Determine the pH of a solution that is 0.50 M in Ch3COOH and 0.75M in NaCH3COO Ka for CH3COOH =…

A: Given:- Determine the pH of a solution that is 0.50 M in Ch3COOH and 0.75M in NaCH3COO Ka for…

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

What volume of 0.1543 M NaOH must be added to 25.00 mL of 0.2405 M HCOOH in
order to prepare a solution of pH =3.7? Explain and justify any simplifying assumptions
made in your calculation.
%3D
KA of HCOOH=1.8 x 104 M

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 with 1 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

Calculate the pH of a solution containing 0.70 M HC2H3O2 and 0.25 M NaC2H302. The K, for HC,H;0, is 1.8x10-5. pH =
How many moles of NH3 would need to be added to 512.9 mL of a 0.25 M solution of NH4Cl to produce a solution with a pH equal to 9.4?
calculate the ph of a solution containing 0.20 M HC2H3O2 and 0.30 M NaC2H3O2The Ka for HC2H3O2 is 1.75 x 10^-5, Then calculate the pH of the acid in pure water
The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to 10 times its original volume? 0.10 M HCI 0.10 M NAOH 0.10 M CH3COOH 0.10 MCH3COO Na" A mixture of 010 M CH;COOH and 0.10 M CH3COO'Na*
Calculate [OH] in a solution obtained by adding 1.90 g solid KOH to 1.00 L of 10.0 M NH3. (Kb of NH3 is 1.80 x 10-5).
50mL of a 2.0M HCl solution is diluted to 6,000mL with distilled water. what is the pH of the resulting solution?
A solution is made by adding 0.320 g Ca(OH)2(s), 35.0 mL of 1.10 M HNO3 and enough water to make a final volume of 75.0 ML. Assuming that all of the solid dissolves, what is the pH of the final solution?
When 46.5 ml of 0.100 M Ba(OH)2 is mixed with 290.7 ml of 0.200 M HCI, the reaction goes to completion. Calculate the pH of the solution. Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to two (2) decimal places. Possibly helpful equations: pH = -log(H'] [H*]= 10- pH Kw =[H*] [OH ] Kw = 1.0 x 10-14 Answer:
How many moles of NH4Cl would need to be added to 441.6 mL of 1.43 M NH3 to produce a solution with a pH equal to 8.66?
I am unsure on how to solve this problem, and it requires not use the H+ approximation where it equals 0.05M and pH=1.301. I would appreciate if I can get some help showing how to solve this problem without using the approximation. (1) Calculate the pH of water containing 0.05 M HCI + 0.05 M KCI, do not use the approximation [H+ ] = aH+
Please don't provide handwriting solution
Please answer these questions on your Page 9 We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.11. We titrate this solution with a 0.166 M NaOH solution and we need 22.2 mL of this NaOH solution to reach the equivalence point. The temperature is 25.0°C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, K₁, of A-(aq)? (c) What was the pH of the solution after the addition of the first 15.0 mL of the NaOH solution?