Answered: Describe how you would make 4 liters of…

Describe how you would make 4 liters of a 0.075 M phosphate buffer at pH of 7.15 without using a pH meter, if the only materials you have are a 1.0 M stock solution of KH2PO4 and a 1M NaOH solution.

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: If I have a buffer solution made up of 25.0 mL of 0.500 M sodium acetate (NaCH3COO) and 25.0 mL of…

Q: Determine the pH of a buffer formed by dissolving 20.0 g NaCH₃COO into a 500.0 mL solution of 0.150…

A: Henderson equation for the calculation of pH of a buffer consisting of a weak acid and salt of the…

Q: 29. The acid HA has an ionization constant of 10-5, If 50 ml 0.1N HA is diluted to 200 ml and…

A: Ka (HA) = 10-5 pKa = -logKa = -log ( 10-5 ) = 5Initial Normality of HA =M1 = 0.1…

Q: Calculate the pH in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid (Ka = 9.8 × 10−5) with…

A: Given : 40 mL of 0.100 M barbituric acid (Ka = 9.8 × 10−5) 29.3 mL of 0.100 M KOH To find : pH…

Q: A 100 mL buffer solution consists of 0.60 M lactic acid (HC3H503) and 0.60 M lactate ion (C3H5O3).…

Q: Calculate the pH of a buffer prepared by adding 0.44 moles of acetic acid and 0.25 moles of acetate…

Q: Draw the Lewis Dot structure for the following diprotic acid: HOOC-(CH2)2-COOH. 46.3 mL of a 0.099 M…

A: Given that : We have to draw the Lewis Dot Structure for the following diprotic acid:…

Q: Part A: A 252-mL buffer solution is 0.420 M in ammonia (NH3) and 0.303 M in ammonium chloride…

A: We would use Henderson Hasselbalch equation to calculate initial pH. Then , HBr which is a strong…

Q: of the following substances, when added to a solution of Chlorous acid (HClO2), could…

A: A buffer solution is defined as solution which resistance to change in it's pH value even when small…

Q: What is the pH for the solution made from 11.10 mL of 0.2780 M NaOH solution mixed with 70.20 mL of…

A: Step 1: Volume of NaOH = 11.10 mL = 0.0111 L.Concentration of NaOH = 0.2780 M.Volume of ammonium…

Q: The pH of a buffer can be calculated using the formula: 14-pOH = pKb + log of [proton…

Q: What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.100 mol of CH₃NH₃I?

A: Given- Moles of CH3NH2=0.580mol Moles of CH3NH3I=0.100mol Kb=4.4×10-4

Q: A 1.0-L buffer solution contains 0.300 mol acid, HA, and 0.300 mol base, NaA. The value of K, for…

A: Weak acid and its salt with strong base will make a buffer whose PH can be calculated with the help…

Q: The pK, of hypochlorous acid is 7.530. A 56.0 mL solution of 0.121 M sodium hypochlorite (NaOCI) is…

A: Answer: In this question we have to calculate the pH of three types of solutions at three different…

Q: 1. Buffers are made from weak conjugate acid-base pairs. In Part A, step 4, of the procedure a weak…

A: Given preparation of buffer solutions. An acidic buffer solution can be prepared by the following…

Q: Calculate the pH of a buffer solution made by mixing 300 mL of 0.3 M acetic acid, CH;COOH, and…

A: Given, a buffer solution is made by mixing 300 mL of 0.3 M acetic acidand 200 mL of 0.2 M of its…

Q: Calculate the pH in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid (Ka = 9.8 × 10−5) with…

A: We will first calculate the concentration of acid and salt. Salt is formed when we add KOH to the…

Q: A student is trying to prepare a buffer solution with a pH of 9.00. Calculate the mass of potassium…

A: pH of a buffer is calculated using Henderson -Hasselbalch equation pH = 9 pka = -log Ka We…

Q: An analytical chemist is titrating 226.3 mL of a 0.3900M solution of hydrazoic acid (HN3) with a…

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

Q: The concentration of H3O+H3⁢O+ in the buffer prepared in the previous question is 2.27×10−5…

A: Since, Negative logarithm of concentration of H+ ion is known as pH of the solution. i.e. pH =…

Q: Given two buffer solutions: Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO Buffer 2 :…

A: The buffer solutions given are, Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO Buffer 2 :…

Q: а.) к.с В.) ноћн -CH₂ D.) H₂C H CH₂ c.) CH Н.С. H d.) CH₂ e.) CH₂ Н

Q: Determine the pH of a buffer that is 0.55 M HNO₂ and 0.75 M KNO₂. The value of Ka for HNO₂ is 6.8 ×…

A: Acid & its salt forms acidic buffer.

Q: An analytical chemist is titrating 60.6 mL of a 0.3000 M solution of butanoic acid (HC,H,Co,) with a…

A: Given : Concentration of HC3H7CO2 = 0.3000 M Volume of HC3H7CO2 solution = 60.6 mL = 0.0606 L…

Q: A buffer solution is made that is 0.319 M in HCN and 0.319 M in NaCN. (1) If Ka for HCN is…

Q: A 1.00 L solution contains 0.372 M HA (Ka = 2.93⋅10−62.93⋅10-6) and 0.741 M NaA. What is the pH…

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

Q: Classify whether it is an organic compound or inorganic compund. Water Salt Sugar

A: Since you have posted a question with multiple sub-parts, we are entitled to answer the first three…

Q: What is the pH of a buffer made from 0.180 mol of HCNO (Ka = 3.5 × 10⁻⁴) and 0.410 mol of NaCNO in…

Q: Calculate the pH of a buffer solution containing 0.659 mol HA weak acid and 0.602 mol A- in 288.3 mL…

A: We have to calculate the pH of solution

Q: You want to prepare a buffer solution with pH equal to 3. How many grams of NaF (41.99 g/mol) should…

A: In this, we need to find oute moles of NaF first. Using that moles and molar mass for NaF, calculate…

Q: A buffer solution is made that is 0.460 M in HCN and 0.460 M in NaCN. If Ka for HCN is 4.00 × 10¬10,…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

A: Henderson-Hasselbalch equation, Is an equation which shows the relationship between the pH and pOH…

Q: What is the pH of a buffer made by combining 45.0 mL of 0.150 M nitrous acid and 20.0 mL of 0.175 M…

Q: You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH;COOH) and 0.30 M sodium…

A: Given: The volume of the buffer solution (V) = 500.0 mL = 0.5 L The concentration of acetic acid…

Q: Calculate the pOH of 103.16 mL of a buffer initially consisting of 0.1752 M H2NCH2COOH and 0.1573 M…

Q: If I have a buffer solution made up of 5.0 mL of 0.500 M sodium acetate (NaCH3COO) and 45.0 mL of…

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: For 480.0 mL of a buffer solution that is 0.120 M in HC2H3O2 and 7.50×10−2 M in NaC2H3O2 , calculate…

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

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: A buffer is prepared from 60.0 mL of 0.100 M formic acid (HCOOH) and 40.0 mL of 0.100 M formate…

Q: Consider a buffer made from 255 mL 0.10 M HC2H3O2 and 125 mL 0.10 NaC2H3O2. Ka for HC2H3O2 is 1.8 x…

A: Moles of HC2H3O2 = Molarity × Volume = 0.10 M ×0.255 L Moles of…

Q: Calculate the pH of a buffer made up by adding 0.65 mol of NaC2H3O2 (sodium acetate) to 00L of a…

Q: The pK, of hypochlorous acid is 7.530. A 60.0 mL solution of 0.123 M sodium hypochlorite (NaOCI) is…

A: we have to calculate the pH of the solution after given amount of HCl is added

Q: You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium…

A: Hey, since there are multiple sub parts posted, we will answer first three questions. If you want…

Q: Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL…

A: It is based on the concept of buffer Here we are required to find the pH of the buffer solution…

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

Describe how you would make 4 liters of a
0.075 M phosphate buffer at pH of 7.15 without
using a pH meter, if the only materials you have
are a 1.0 M stock solution of KH2PO4 and a 1M
NaOH solution.

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

Name the alkenes below. Use ONLY E/Z designators to indicate stereochemistry. H3C H Ja H CH₂-C H CH3 CH₂CH3
A 350-mL buffer solution is 0.500 M in chlorous acid (HClO2, Ka=1.1×10−2) and 0.200 M in sodium chlorite (NaClO2). What is the pH of this solution? Express your answer using two decimal places.pH =
A buffer solution is 0.463 M in H3PO4 and 0.210 M in KH₂PO4. If K₁1 for H3PO4 is 7.5 × 10-³, what is the pH of this buffer solution? pH =
Calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer solution that is 0.2604 M in CH3CH2NH2 and 0.2404 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Kb=5.6⋅10^−4).
What is the pH after 15.0 mL of 0.200 M NaOH has been added to 100.0 mL of a buffer solution consisting of a weak base, X, with a concentration of 0.80 M and its conjugate acid, HX+, with a concentration of 0.55 M if the weak base ionization constant, Kb, is 3.3 x 10−5?
Phosphoric acid is a triprotic acid (?a1=6.9×10^3Ka1=6.9×10^3, ?a2=6.2×10^8 Ka2=6.2×10−8, and ?a3=4.8×10^13Ka3=4.8×10^13). Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH2PO4(s) and 30.0 g of Na2HPO4(s) in water and then diluting to 1.00 L. pH=
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)
How many grams of dry NH4Cl need to be added to 2.50 L of a 0.300 M solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.74? Kb for ammonia is 1.8×10−5 . (Please type answer no write by hend)
6. After adding NH3 (g) to a buffer solution consisting of the conjugate acid/base pair: NH4*/NH3 (without changing the solution volume), which of the following statements is true? K, (NH¼*) = 5.6 x 10 1º. a) The pH of the solution will decrease. b) The concentration of H3O* will increase. c) The concentration of NH4 will increase. d) none of the above
Could you explain how to know which one will have a pH>7
A chemist needs a buffer with pH 4.34. How many milliliters of pure acetic acid (density = 1.049 g/mL) should Dimitry add to 325.0 mL of 0.2633 M NaOH solution to obtain such a buffer?
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 100.0 mL of the strong base has been added. The value of Ka for HC4H;O2 is 1.5 × 10-5 1 2 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC4H;O2(aq) + OH (aq) H20(1) + C4H,O2 (aq) Before (mol) |Change Imol) After | (mol) RESET 0.100 0.200 +x 0.100 + x 0.100 - x -x 0.200 + x 0.200 - x 2.00 x 103 -2.00 x 103 8.00 x 103 -8.00 х 10"3 1.00 x 102 -1.00 x 102 1.20 х 10"2 -1.20 x 102 2.00 x 10-2 -2.00 x 102