How many milliliters of 1.79 M NaOH must be added to 175 mL of 0.14 M H2PO4 to make a buffer solution with a pH of 7.70? Be sure your answer has the correct number of significant digits. Note: Reference the pK of weak acids at 25 °C table for additional information.

How many milliliters of 1.79 M NaOH must be added to 175 mL of 0.14 M H2PO4 to make a buffer solution with a pH of 7.70? Be sure your answer has the correct number of significant digits. Note: Reference the pK of weak acids at 25 °C table for additional information.

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: uppose a solution of NaOH was titrated and found to have a molarity of 0.250 M. This solution is now…

Q: What is the pH of a buffer solution prepared from 0.411 moles of CH3COOH and 0.457 moles of NaCH3COO…

Q: Calculate the change in pH when 4.00 mL of 0.100 M HC1(aq) is added to 100.0 mL of a buffer solution…

Q: A solution is prepared that is initially 0.35M in hydrocyanic acid (HCN) and 0.22M in potassium…

A: The objective of the question is to complete the reaction table for the given solution of…

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: A buffer is prepared by using 0.20 mole of C6H5COOH and 0.40 mole of C6H5COO- in 1.00 liter of…

A: The objective of this question is to determine whether the buffering capacity of a solution,…

Q: A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol…

A: Given, Volume of HCl = 44.6 mL = 0.0446 L (1mL = 0.001 L) Molarity of HCl = 0.103 M = 0.103 mol/L…

Q: Determining the pH of Buffer Solutions Imagine you are given 50.0 mL of a 0.50 mol/L solution of…

Q: A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)¸N) ³ N) solution with 0.8123 M HCl…

A: Concentration of trimethylamine = 0.2187 MVolume of trimethylamine = 110.0 mLpKb of triethylamine =…

Q: Calculate the pH of a solution that is 0.080 M pyridine (pKb = 5.25) and 0.215 M pyridinium…

A: A buffer solution is a solution that resists a change in its pH on the addition of a small amount of…

Q: What will be the pH of the buffer solution consisting of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189…

Q: Consider a 1.0-L solution that is 0.280 M C5H5N and 0.46 M C5H5NHCl at 25 °C. What is the pH of this…

A: The question is based on the concept of PH calculation. using henderson equation, we calculate…

Q: A 0.100 L solution is composed of 0.500 M (CH3)2NH and 0.500 M (CH3)2NH2Cl at 25 oC. What is the pH…

A: The objective of the question is to calculate the pH of the solution after the addition of .A buffer…

Q: An buffer is prepared by combining 1.61 moles of HX solution with 0.28 moles NaX and diluting to a…

A: Given :- number of moles of HX = 1.61 mol Number of moles of NaX = 0.28 mol Total volume = 1 L Ka…

Q: Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2…

A: From the balanced chemical reaction between HCl and Na2CO3, we can solve these problems. 2HCl +…

Q: 10mL of solution B has 10mL of water added to it, how does this effect the pH - what two solutions…

A: #Part-1: 10 mL solution-B + 10 mL water: # pH before the addition of water: Dissociation equation of…

Q: Calculate the pH of a buffer solution made by mixing 185.8 mL of a 1.56 M propanoic acid…

Q: An analytical chemist is titrating 187.2 mL of a 0.7600M solution of butanoic acid (HC3H7CO2) with a…

A: To calculate the pH of the solution during the titration, we can follow these steps:1. Calculate the…

Q: Which of the following solutions will have the greatest buffering capacity given the following…

A: Given Solution 1. 0.6M HCN and 0.7M KCN2. 0.5M HCN and 0.9M NaOH3. 0.9M HCN and 1M CNOH4. 0.2 M HCN…

Q: A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Step 1:Solution of weak acid and its conjugate base can only act like a buffer solution when ratio…

Q: A solution is made with 554 ml of 8.21 M HX solution and 549 mL of 6.06 M Nax solution and the pH at…

Q: Consider the following reaction: CH3COOH(aq)+OH−(aq)CH3COO−(aq)+H2O(l) See Periodic Table…

Q: An analytical chemist is titrating 150.4 mL of a 0.5000M solution of benzoic acid (HC H-CO₂) with a…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: A chemistry student weighs out 0.270 g of citric acid (H;C,H;0;), a triprotic acid, into a 250. mL…

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: When 22.6 mL of 0.229 M hydrochloric acid (HCI) and 22.6 mL of 0.229 M ammonia (NH3) are combined,…

Q: How many mL of 0.13 M NaOH have to be added to reach the equivalence point when 15.00 mL of 0.14 M…

A: Here 3H+ neutralizing with 1OH- thus the formula is:- 3M1V1(NaOH)= M2V2(H3PO4)

Q: pose 26.5 mL of 0.19 M NaOH is added to 45.3 mL of 0.24 M HCHO2. What will be the pH of the…

A: Molarity of HCOOH= 0.24 M Volume of HCOOH= 45.3 ml Molarity of NaOH = 0.19 M Volume of NaOH =…

Q: A chemist titrates 50.0 mL of a 0.4918M hydrocyanic acid (HCN) solution with 0.8729M KOH Solution at…

A: First we will determine the concentration of salt at equivalance point. Since it's a titration of…

Q: The next 11 questions are related to the titration of 40.00 mL of a 0.0900 M acetic acid solution…

Q: Calculate the pH change that results when 15 mL of 2.6 M HCl is added to 600. mL of each of the…

A: 1) Let us find the number of moles of HCl Total Volume = 15 mL + 600 mL = 615 mL

Q: How many mL of 0.24 M NaOH have to be added to reach the equivalence point when 15.00 mL of 0.24 M…

Q: For 480.0 mLmL of a buffer solution that is 0.160 M� in CH3CH2NH2CH3CH2NH2 and 9.00×10−2 M� in…

A: The objective of the question is to calculate the initial and final pH of a buffer solution after…

Q: An analytical chemist is titrating 79.7 mL of a 0.4500M solution of ammonia (NH3) with a 0.1600M…

Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has…

Q: An analytical chemist is titrating 101.8 mL of a 1.100M solution of benzoic acid (HC HCO₂) with a…

A: A solution of benzoic acid 1.100M x 101.8ml = 111.98 mmol is titrated with 0.2600 M × 514.6 ml =…

Q: Which of the following solutions will h

A: the solutions which resists change in pH by the addition of small amount of strong acid (or) base…

Q: calculate the 10.0 mL of 0.10 M KOH is added to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10–10). Find the…

Q: A 1.0m HCl solution has a volume of 20.0mL. Calculate pH of the solution that results from 3.00g of…

A: Given: Molarity of HCl solution= 1.0 M Volume of HCl= 20.0 mL= 0.020 L Mass of solid acetate= 3.00 g…

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

How many milliliters of 1.79 M NaOH must be added to 175 mL of 0.14 M H2PO4 to make a buffer solution with a pH of 7.70? Be sure your answer has the
correct number of significant digits.
Note: Reference the pK of weak acids at 25 °C table for additional information.
a

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: Determine the volume of NaOH from the given data:

VIEW

Step 2: Calculation for volume of NaOH :

VIEW

Solution

VIEW

Step by step

Solved in 3 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

consider the titration of 50.0 mL of 0.10 M acetic acid with NaOH. drag and drop each amount of NaOH added (to the acetic acid) Into the appropriate resulting pH. In other words, determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solutions be acidic, basic, or neutral? Consider the stration of 50.0 ml of 0.10 M acetic acid (HC₂H₂O₂. K, -18 x 10) with NaOH. Drag and drop each amount of NaOH added to the acetic acid) into the appropriate resulting pH. In other words determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solution be acidic, basic, or neutra? Acidic Neutral Basic Drag and drop your selection from the following list to complete the answer 25.0 mL (total) of 0.10 M NaOH has been added (the halfway point) 50.0 mL. (total) of 0.10 M NaOH has been added (the equivalence point) 10.0 mL (total) of 0.10 M NaOH has been added 60.0 mL (total) of 0.10 M NaOll has been added No NaOH has been…
Calculate the pH of a solution that is 0.080 M pyridine (pKb = 5.25) and 0.285 M pyridinium chloride.
5 What volume, in milliliters, of 0.240 M NaOH should be added to a 0.135 L solution of 0.030 M glycine hydrochloride (p Kal = 2.350, pKa2 = 9.778) to adjust the pH to 2.78? 5 NaOH volume = mL
How many grams of lactic acid and mL of 0.1M sodium hydroxide must be added to 100 mL of water to produce a solution with pH 3.9 and a total solute concentration of 0.25, 0.5, and 0.1mM?
What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and 0.2 mol of acetic acid (HC2H3O2) in enough water to give 1.00 L solution? Ka for acetic acid = 1.8 x 10-5 .
It says that my answers are wrong but it won’t tell me what answers are wrong I thought I did it right please help me.
A 0.500 L solution is composed of 0.200 M (CH3)2NH and 0.200 M (CH3)2NH₂Cl at 25 °C. What is the pH of the solution after 0.040 moles of HBr are added to the solution at the same temperature? You may assume no change in volume for the system. Enter your answer with two decimal places. At 25 °C: Kb for (CH3)₂NH = 5.9 x 10-4 Kb for KOH= 3.2 x 10¹
An analytical chemist is titrating 169.4 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 1.100M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 183.1 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ☑
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 3.2–3.5 a - NaNO 2 / HNO 2 (K a = 4.5 × 10 –4) b - NaOCl / HOCl (K a = 3.2 × 10 –8) c - NaCl / HCl d - NH 3 / NH 4Cl (K a = 5.6 × 10 –10) e - CH 3COO 2Na / CH 3COOH (K a = 1.8 × 10 –5)
An analytical chemist is titrating 146.0 mL of a 1.200 M solution of benzoic acid (HC6H5CO₂) with a 0.6900 M solution of NaOH. The pK of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 46.25 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0 ×
Suppose 85 mL of a buffer solution that was 0.15 M HCHO2 and 0.25 M NaCHO₂ had 7.5 mL of 0.10 M hydrochloric acid added to it. Afterwards, 35 mL of this mixture was measured out, placed inside an Erlenmeyer flask, and diluted to 75 mL. What was the concentration of the hydroxide ion in the resulting solution in the flask? Ka for HCHO2, formic acid, is 1.7 x 10-4. a. 9.80 x 10-11 M Ob. 2.81 x 10-7 M c. 2.55 x 10-9 M d. 8.94 x 10-11 M e. 2.10 x 10-10 M 9.77 x 10-11 M g. 1.12 x 10-4 M Incorrect Of. Oh. 1.91 x 10-10 M
What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL of aqueous ammonia (NH3) requires 37.10 mL of 0.1087 mol L-1 HCI? pK₁ =4.75 for ammonia. Report your answer in 2 decimal places.