10 Of the following solutions, which has the greatest buffer capacity (assuming 1 L of each)?0.050 M HNO2 and 0.120 M NaNO20.650 M HNO2 and 0.790 M NANOO 0.180 M HNO2and 0.180 M NaNO0.400 M HNO2 and 0.385 M NaNOThese are all buffer solutions and would all have the same capacity.acer2.2.2.

Buffer solutions resist tochange in pH According to Henderson pH of acidic buffer is pH = pKa…

Answered: Of the following solutions, which has…

Of the following solutions, which has the greatest buffer capacity (assuming 1 L of each)? O 0.050 M HNO2 and 0.120 M NANO2 0.650 M HNO 2 and 0.790 M NaNO 2.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.99E

See similar textbooks

Related questions

Q: Calculate the pH of a buffer containing 0.1 M HC2H3O2 (aq) mixed with 0.1 M NaC2H3O2 (aq)?

A: The buffer solution will contain 0.1 M acetic acid (weak acid) and 0.1 M sodium acetate (salt of…

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

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

Q: What is the pH of a buffer prepared by combining .92 moles of a weak base B, with .59 moles of…

Q: You have a 0.500 L buffer solution composed of 0.47 M formic acid (HCOOH, Ka = 1.77 x 10¯4) and…

A: The acid ionization constant for acid is 1.77×10 -4.

Q: A 1.000 L buffer solution contains 0.250 mol/L NH, and 0.250 mol/L NH,Cl. K = 1.8 x 10* Determine…

Q: Define buffering capacity. How do the followingbuffers differ in buffering capacity? How do they…

A: Value of pH is used to determine whether the solution is acidic or basic in nature. At room…

Q: Which of the compounds is more soluble in an acidic solution than in pure water? AIPO4 O CSCIO4 Cas…

Q: Which of the following are capable of forming a buffersolution?a. HBr and MgCl2b. H2CO3 and NaHCO3

A: Correct answer is (b) H2CO3 and NaHCO3 . Buffer solution should contain weak acid and its salt with…

Q: How many grams of dry NH4Cl need to be added to 2.40 L of a 0.800 M solution of ammonia to prepare a…

Q: How many microliters of 1.000 M NaOH solution mustbe added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: estion 2 Of the following solutions, which has the greatest buffering capacity? 0.543 M NH3 and…

Q: Calculate the change in pH when 43.0 mL of a 0.760 M solution of NaOH is added to 1.00 L of a…

A: The volume of 43 mL is equivalent to 0.043 L. To determine the number of moles (n) of NaOH in the…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has:Concentration of NH4Cl/NH4+ = 0.181 MConcentration of NH3 =…

Q: How many microliters of 1.000 M NaOH solution must be added to 25.00 mL of a 0.1000 M solution of…

A: Find the moles of lactic acid.

Q: 8. A 1.000 L buffer solution contains 0.250 mol/L. NH, and 0.250 mol/L. NH, CL K=1.8x10 Determine…

A: We have to calculate the pH

Q: What is the pH of a buffer made from 0.350 mol of HBRO (Ка 3 (Ka = 2.5 x 10°) and 0.080 mol of KBRO…

A: Given : Moles of HBrO = 0.350 mol. Moles of KBrO = 0.080 mol. Ka of HBrO = 2.5 X 10-9 And volume of…

Q: Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate,…

Q: I have attached a picture of a problem that I'm having a hard with. Could you help and break down…

A: Buffer solutions are the solutions which resist the change in pH when small amount of acid or base…

Q: Which of the following salts would be more soluble in acidic solution than in neutral water? A.…

A: The dissolving capacity of any component in fix amount of liquid is referred as solubility and the…

Q: Which of the following buffer solutions has the highest buffer capacity A. 0.10 M NHz and 0.10 M…

A: An acid or a base is described as a weak acid or a weak base based on the amount of the dissociation…

Q: A 27.0-mL solution of 0.120 M CH3COOH is titrated with a 0.230 M KOH solution. Calculate the pH…

Q: What is the pH of a buffer solution made by adding 0.020 mole of solid NaF to 100. mL of 0.40 M HF?…

Q: Which of these substances are more soluble in acidic solution than in basic solution:(a) Ni(OH)2(s),…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Consider a buffer made by adding 132.8 g of NaC,H;O2 to 300.0 mL of 1.31 M HC,H;O2 (Ka = 6.3 x 105)…

Q: A 28.0-mL solution of 0.120 M CH3COOH is titrated with a 0.220 M KOH solution. Calculate the pH…

Q: What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (K, = 1.8 x 10$)?

A: Given : Concentration of weak acid CH3COOH = 0.15 M And concentration of conjugate base salt of weak…

Q: A volume of 500.0 mL of 0.160 M NAOH is added to 545 mL of 0.200 M weak acid (Ka = 6.62 x 10-). What…

A: pH = pKa + log[salt]/[acid] pKa = -logKa

Q: What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10⁻⁹) and 0.160 mol of KBrO in…

A: For HBrO , pKa = -log Ka = -log ( 2.5 × 10⁻⁹ ) = 9 - log2.5 = 9 - 0.40 = 8.60 For buffer : pH = pKa…

Q: 1. What is the pH of a buffer that contains 0.15 M CH,COOH and 0.10 M NACH,COO (K, = 1.8 x 10 )?

A: 1) Given, Concentration of CH3COOH solution = 0.15 M [CH3COOH] = 0.15 M Concentration of NaCH3COO…

Q: Calculate the buffer capacity of the following solutions: . A mixture of 0.1 M CH3COOH and 0.1 NaOH…

Q: A chlorous acid buffer containing 0.75 mol of HCIO₂(aq) and 0.75 mol of NaClO₂(aq) in 1.00 L has a…

A: we have to calculate pH of the buffer solution

Q: Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate,…

Q: A buffer solution contains 0.200 M CH3NH2 and 0.250 M CH3NH3Cl. What is the pH of the buffer…

A: The number of moles of methylamine in 50 mL buffer solution is calculated as follows:

Q: What is the pH of the buffer 0.1 M Na2HPO4/0.15 M KH2PO4?

Q: A volume of 500.0 mL of 0.160 M NAOH is added to 545 ml. of 0.250 M weak acid (K, = 8.52 x 10-5).…

Q: Alkalimetric titrant can be: KOH solution; H2SO4 solution; NH,OH solution; CH;COOH solution

A: Alkalimetric titration are used to determine the quality of a base in a solution

Q: 10- Which of the following can be classified as buffer solutions? a. 0.25 M HBr + 0.25 M HOB1 b.…

A: A buffer is a solution that contains a mixture of a weak acid and its conjugate base, or a weak base…

Q: Calculate the pH of the following two buffer solutions: (a)2.0 MCH3COONa/2.0 M CH3COOH, (b) 0.20 M…

A: The pH of a acidic buffer can be calculated as follows: pH=pKa+logSaltAcidwhere Ka is the…

Q: A chemistry graduate student is given 250. mL of a 0.60 M nitrous acid (HNO,) solution. Nitrous acid…

A: Since HNO2 is a weak acid. Hence on dissolving its salt i.e NaNO2 , the solution will have weak acid…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has: Concentration of NH4Cl/NH4+ = 0.182 M Concentration of NH3…

Q: Calculate the concentration of ions in the following saturated solutions: (a) [I] in AgI solution…

Q: A buffer solution that is 0.397 M in HCN and 0.397 M in KCN has a pH of 9.40. The addition of 0.01…

A: Given that, We have a buffer solution containing 0.397 (M) HCN and 0.397 (M) KCN. The buffer…

Q: er soluble ions produced by the addition of Na2O2 and ex

A: The chemical reaction between Na2O2 and excess KOH is given below: Na2O2 + 2KOH → 2NaOH + 2KO.

Q: A titration is performed in which 0.14 M KOH is added to a 150.0 mL sample of 0.39 M HI. What is the…

A: PH of KOH can be calculated as follows

Q: Calculate the concentration of ions in the following saturated solutions. (a) [I-] in AgI solution…

A: The solubility product constant, Ksp, is the equilibrium constant for a solid substance dissolving…

Q: Which salts will be more soluble in an acidic solution than in pure water? Sn(OH)2 AgBr KClO4 CaCO3…

A: The fact to these is knowing what anions react with H^+ (the acid) and if any weak acids or…

Q: A buffer is prepared by mixing 25 mL of 0.10 M nitrous acid (HNO2) and 25 mL of 0.15 M sodium…

Q: A volume of 500.0 mL of 0.160 M NaOH is added to 545 mL of 0.250 M weak acid (K, = 5.89 x 10-5).…

A: The PH of acidic buffer can be calculated as follows

Q: What is the pH of a buffer composed of 0.45 M C5H10NH and 0.65 M [C5H10NH2]Cl?

A: Formula for calculating pOH of a solution consisting of a weak base and its salt with a strong acid:…

Concept explainers

Matter and Measurement

In the universe, there is matter, energy, and void space. The universe contains energy and void space. The definition of matter can be considered as something which possesses mass and consumes space. Chemistry is that branch of science which deals with the study of matter. Under chemistry, nature, composition, and the changes occurring to matter are discussed.

Question

Of the following solutions, which has the greatest buffer capacity (assuming 1 L of each)?
0.050 M HNO2 and 0.120 M NaNO2
0.650 M HNO
2 and 0.790 M NANO
O 0.180 M HNO
2
and 0.180 M NaNO
0.400 M HNO
2 and 0.385 M NaNO
These are all buffer solutions and would all have the same capacity.
acer
2.
2.
2.

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 Acidic Buffer

VIEW

Step 2 Explanation

VIEW

Step 3 Conclusion

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
Calculate the solubility (in grams per liter) of silver chloride in the following. (a) pure water (b) 0.025 M BaCl2 (c) 0.17 M AgNO3
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.
Three acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2 Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3 Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). b When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization?
Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?
Use the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. a AgBr b Ca(NO3)2 c MgI2 d PbSO4
If 13.50 mL of an aluminum chloride solution is needed to reach the equivalence point with 10.00 mL of 0.109M silver nitrate solution determine the molarity of the aluminum chloride solution. here I chemical balanced the equation AICl3 + 3AgNO3 = 3AGCl + Al(NO3)3 Please can you help me with this question? My homework solutions are always answered late next days instead of one hour. I don't get my homework solutions on time like withing one hour.
a. An aqueous solution contains 0.20 M hydrocyanic acid.One Liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.21 mol KCN 0.21 mol HI 0.20 mol KBr 0.050 mol Ba(OH)2 0.10 mol HI b. An aqueous solution contains 0.18 M ammonium iodide. One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.18 mol HNO3 0.17 mol KI 0.08 mol HNO3 0.08 mol KOH 0.17 mol NH3 c. An aqueous solution contains 0.33 M sodium fluoride.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.16 mol KOH 0.33 mol HCl 0.32 mol NaCl 0.32 mol HF 0.16 mol HCl
A student performed a redox titration of 10 mL samples of acidified tin(II) chloride solution, with standardized KMnO4(aq) as the titrant in a burette. Calculate the concentration of the acidified tin(II) chloride solution if 17.4 mL of 0.100 mol/L of standard potassium permanganate solution was used. Select one: O a. 0.435 mol/L b. 0.174 mol/L C. 0.0696 mol/L O d. 0.144 mol/L
In a titration of KOH, 0.0725 g of KHP is weighed into a flask and dissolved in deionized water. The equivalence point of the titration is reached when 6.75 mL of KOH is added to the KHP solution. How many moles of KOH will have to be titrated to neutralize the KHP?