Answered: Which pair of substances can form a…

Which pair of substances can form a buffer in aqueous solution? Justify your answer. а. НРО, Na;PO, b. HNO3, NANO3 с. Н.СО, NaNО: d. NH3 and (NH4)2SO4

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: Ba 13. Briefly describe what a buffer is. Include the relevant conceptual background along with…

A: Here we have to brifely describe about Buffer solution and how it react with strong base and acid.

Q: Consider a buffer solution prepared from HOC1 and NaOC1. Which is the net ionic equation for the…

A: A molecular equation is defined as the chemical equation which is written using the chemical formula…

Q: Buffer: HC₂0/C₂O²- What mass of Na2C2O4 must be added to 500. mL of 0.25 M HC2O4- to generate a…

A: Given: Volume of HC2O4- is 500 mL Molarity of HC2O4- is 0.25 M. pH is 4.35.

Q: Buffer solution is made by taking 0.404 moles of acid (Pka=5.83) & 0.468 moles of sodium acetate and…

Q: 16.9 Which of the following solutions can act as a buffer: (a) KCI/HCl, (b) KHSO4/H₂SO4, (c)…

A: Buffer solution is solution contains weak acid or weak base with conjugate base or conjugate acid…

Q: What volumes of 0.200 M HNO2 and 0.200 M NaNO2 are required to make 500. mL of a buffer solution…

Q: A buffer solution contains 0.433 M NaHSO3 and 0.291 M K2SO3. If 0.0340 moles of sodium hydroxide are…

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

Q: [Review Topic IReferences Use the References to access important values if needed for this question.…

Q: How does the buffer react to the addition of acids and bases? In comparison, how does water react to…

A: Buffer solutions are aqueous solutions that resist the change in pH on addition of small amount of…

Q: One function of our blood is to carry CO2CO2 from our tissues to our lungs. It is critical that the…

Q: What volume of 2.00 M NAOH must be added to 150.0 mL of 1.20 M glycolic acid to produce a buffer…

Q: A buffer solution is 0.449 M in HNO, and 0.365 M in KNO, . If K, for HNO, is 4.5×104 , what is the…

A: Introduction : We have to calculate pH of HNO2

Q: Suggest 2 different buffer systems that can be used for the preparation of a pH=7.7 buffer solution?

A: Buffer solution is a solution of weak acid and its conjugate base or weak base and its conjugate…

Q: A buffer solution contains 0.398 M KH₂PO4 and 0.355 M Na₂HPO4 If 0.0248 moles of hydrochloric acid…

A: It is based on the concept of buffer.Here we are required to find the pH of the solution when 0.0248…

Q: Let X represent a nonmetal. Which of the following buffer solutions functions at the lowest pH? More…

A: pH of a buffer consisting of a weak acid and salt of same acid with a strong base can be calculated…

Q: which of the following weak acids would be the best to use to make buffer solution of pH=7.2?

A: A buffer solution is a solution whose pH does not change by adding small amount of acid and base.…

Q: 6. Suppose you have a solution that was prepared by mixing equal amounts of nitric acid (HNO:) with…

A: In this question, we want to explain no more than two sentence that resulting solution is a buffer…

Q: 12. What volume (in mL) of a 0.150 M Na2SO3 solution must be added to 20.0 mL of a 0.120 M NaHSO3…

Q: 3. A buffer solution is created with the following components: 0.067 M HC,H;O, (acetic acid) 0.075 M…

A: This question is related to ionic equilibrium concept. Follow step-by-step solution.

Q: Which of the following solutions can act as a buffer? (a) KCl/HCl, (b) KHSO4/H₂SO4, (c) Na₂HPO4/…

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.339 M hypochlorous acid…

Q: 2) How many grams of NaOH should be mixed with 5.4 g of oxalic acid (H,C.O.) and completed to 100 ml…

Q: definition of bufter solution i - buffer capacity?

Q: 2. Explain the term 'buffer capacity'.

A: Explanation of term "buffer capacity "

Q: A 20.00-mL sample contains 1.00 g of NaHCO,. This sample is used to standardize an N&OH solution. At…

A: a) Calculation of no. of mol of NaHCO3: n=given massMolar mass=1.00 g84.007 g/mol=0.012 mol At the…

Q: Which of the following pairs of substances will make aqueous buffer solutions (consider the products…

A: Acidic buffer: A mixture of weak acid and salt of same acid with a strong base Basic buffer: A…

Q: A 12.7 mL solution of 0.100 mol L-1 HOCI is titrated using 0.150 mol L-1 NaOH. What is the pH of the…

Q: A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, HC7H5O2, and sodium…

A: The objective of this question is to calculate the pH of a buffer solution prepared by dissolving…

Q: 8. What happens if a large amount of a strong acid or base is added to a buffer? Explain. ( C2)

A: In this question, we will explaining you what happened when we adding larger amount of acid or base…

Q: You are given 5.0 gram of an unknown sample is titrated via 0.125N standard HCl. Volume of titrant…

Q: d. Oxalic acid (H2C2O4) is the compound that gives rhubarb its tart flavor, and it is also a toxin…

A: The question is based on the concept of molarity.Molarity is a method of expressing concentration of…

Q: HW9 #16

A: Before analyzing the given statements, there must be the basic understanding of buffer…

Q: Determine the mass of H2C2O4.H2O required to prepare 0.1N solution in 100 ml volume. Explain two…

A: Hi, since you have posted multiple questions, we will answer the very first question for you. Kindly…

Q: Which of the following solutions can be classified as buffer systems? (a) KH,PO/H;PO4 (b)…

A: Buffer solution are those solutions which resist a change in pH upon addition of small amount of…

Q: 2) Which of the following combinations of materials would result in a buffer solution? *100. mL of…

A: A buffer solution is a solution that can resist changes in pH when small amounts of acid or base are…

Q: 1- Which of the following mixtures is not a buffer and calculate its pH: (K,=K, =1.8 x 10) a. 25ml 0…

A: 1.Buffer solution mean a solution that retard the change of pH when H+ or OH- is added, in buffer…

Q: Supplemental Question Q8 (to be answered under section C) Regarding your answers in the fifth column…

A: A question based on equilibrium concept that is to be accomplished.

Q: The assigned buffer will be a 0.10 M, pH 6.70 buffer. The only available reagents are: 0.20 M…

A: We need to prepare the buffer with pH 6.70.

Q: 7. Which pH is consistent with the following results? Indicator Color result Thymol blue yellow…

Q: 2- Calculate the pH of the following buffer solutions: a) 0.0405 M NH,OH + 0.02 M (NH4);SO, . b)…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: A student is asked to prepare a buffer solution at pH = 8.60, using one of the following weak acids:…

A: Given : pH = 8.60

Q: created by combining 3.45 g of NH, of HCI and diluting to a total volume of

Question

Which pair of substances can form a buffer in aqueous solution? Justify your answer.
а. НРО, Na;PO,
b. HNO3, NANO3
с. Н.СО, NaNО:
d. NH3 and (NH4)2SO4

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

20.3 mL of 0.144 M solution of nitric acid is titrated with 0.106 M NaOH solution. What is the pH before any base solution is added?
The addition of hydrofluoric acid, HF and, to water produces a buffer solution? O NaNO3 NaCl NaF HCI ONaBr
H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion
Which of the following constitute a buffer? A. NH3 and KNO3 B. HCN & NaCN C. HF & NaCl D. NaOH & NaCl Group of answer choices C A & C B A, B and C
Describe/ explain what a buffer is/ how it works. Do Not use the words "acid" or "base" or any derivative of those (e.g. "acidic", "basic", etc.)?
A volume of 25.0 mL of 2.75 M HCl, is to be titrated with 1.025 M strong base, B(OH)2. Calculate the ff: A. pH of the resulting solution when the original solution has been titrated with 50.0 mL of the base titrant. B. pH of the resulting solution when the original solution has been titrated with 60.0 mL of the base titrant. C. pH of the resulting solution when the original solution has been titrated with 70.0 mL of the base titrant.
4. The molar ratio between a weak acid and its base conjugate was (3:2). Calculate the Ka of the weak acid if the pH of the buffer was 6.0.
A 20.00-mL sample contains 1.00 g of NAHCO,. This sample is used to standardize an NaOH solution. At the equivalence point, 39.60 mL of NaÓH have been added. K,(HCO, ) = 4.8 x 10 Indicators that change color within the pH range: bromothymol blue = 6.0 – 7.7 phenolphthalein = 8.3 – 9.8 alizarin yellow R = 10.0 – 12.0 a. What was the concentration of the NaOH? Concentration M b. What is the pH at the equivalence point? pH = c. Which indicator, bromothymol blue, phenolphthalein, or alizarin yellow R, should be used in the titration? bromothymol blue phenolphthalein allzarin yellow R y Another Version 10 item attempts remaining
ave to.) The K of acetic acid is 1.8 | 10. (Note: solid sodium acetate comes as a hydrate NaC2H3O2 3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer at pH 4.10, given that you will use 5.00 mL of 1.0 M acetic acid.
How many moles of sodium hydroxide would have to be added to 125 mL of a 0.376 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.050? moles
Can you help me with #2
Most carbonates are insoluble in water. Small concentrations of Mg2+ in tap water can react with bicarbonate to create scale deposits inside of tea kettles. a) Show the law of mass action for this interaction. b) Where does the bicarbonate come from in this example? c) Do you expect the solution to become slightly acidic, basic, or neutral due to this interaction? d) How will the molar solubility of magnesium bicarbonate to change if you were to place it into acidic conditions?