A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K2HPO4. Determine the pH changewhen 0.061 mol HCIO, is added to 1.00 L of the buffer.pH change =|A buffer solution contains 0.229 M CGH;NH3CI and 0.381 M C,H3NH2 (aniline). Determine thepH change when 0.077 mol HCl is added to 1.00 L of the buffer.pH after addition – pH before addition = pH change =|A buffer solution is 0.301 M in HCN and 0.274 M in KCN . If K, for HCN is 4.0×10-10 , what isthe pH of this buffer solution?

The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Answered: A buffer solution contains 0.387 M…

A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K,HPO4. Determine the pH change when 0.061 mol HCIO, is added to 1.00 L of the buffer. pH change

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 14QAP: A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to...

See similar textbooks

Related questions

Q: A 20.6 mL sample of 0.377 M methylamine, CH3NH2, is titrated with 0.364 M perchloric acid. After…

A: Number of moles of CH3NH2= M*V = 0.377 M* 20.6 mL = 7.7662 mmol Number of moles of HClO4 = M*V =…

Q: What is the pH of a buffer solution containing 0.21 M HNO2 and 0.10 M NO, ?

A: Since HNO2 is a weak monoprotic acid with pKa = 3.15 And the solution is given buffer solution with…

Q: An aqueous solution contains 0.28 M hydrofluoric acid. One Liter of this solution could be converted…

Q: A buffer solution contains 0.225 M propionic acid, HC3H5O2, and 0.0833 M sodium propanoate,…

Q: Determine the pH when 0.05mole of CO2 is dissolved into 1L of water. When 0.03 mole of sodium…

A: The carbon dioxide is a gas that dissolves n water upto a certain extent. There exists an…

Q: 25 mL of a 0.356 M solution of NH4+ was mixed with 40 mL of 0.842 M potassium nitrate. What is the…

A: Given, Molarity of NH4+ = 0.356 M Volume of NH4+ = 25 mL Molarity of KNO3 = 0.842 M Volume of…

Q: Determine the pH change when 0.075 mol HClo, is added to 1.00 L of a buffer solution that is 0.327 M…

A: When HClO4 added in buffer solution then H+ react with F- ion and form HF

Q: A decrease in pH will increase the solubility of CaCO3 because

A: As acidity increases as PH decreases now, CaCO3 in aqueous solution completely dissociates into…

Q: The addition of Hf and ___ to water produces a buffer solution. KOH KNO3 NaCI HBr NaBr

A: The solutions get prepared through mixing of weak acid+conjugate salt or weak base+conjugate salt…

Q: A 29.4 mL sample of 0.301 M ammonia, NH3, is titrated with 0.317 M hydroiodic acid. At the…

A: The pH at the equivalence point is 4.88

Q: A 30.0 mL sample of 0.200 M HNO, solution is titrated with 15.0 mL of a 0.300 M LIOH solution.…

Q: A 23.1 mL sample of 0.372 M ammonia, NH3, is titrated with 0.354 M perchloric aci After adding 9.93…

A: Kb of NH3 = 1.8*10-5 [source : google] millimoles of NH3 = molarity*volume = 0.372*23.1 =…

Q: The pH of a saturated solution of a metal hydroxide M(OH)2 is 10.500. Calculate the Ksp for this…

A: ksp : sloublity product Ksp = equilibrium between solids and liquids

Q: Use the References to access important values if needed for this question. A 21.4 ml sample of 0.263…

Q: n aqueous solution contains 0.32 M ammonia. One liter of this solution could be converted into a…

A: The Buffer Solution is a chemical compound that resists changing its pH. This buffer solution…

Q: The buffer solution is able to maintain pH by some events, except... * The addition of a little acid…

Q: A buffer solution contains 0.436 M KH,PO4 and 0.317 M K,HPO4. If 0.0156 moles of sodium hydroxide…

Q: Which of the following statement is incorrect regarding buffer solutions: Maximum buffer capacity is…

A: Buffer solution are the mixture of acid and base or acid and its congugate base , it resist the…

Q: A 29.4 mL sample of 0.301 M ammonia, NH3, is titrated with 0.317 M hydroiodic acid. At the…

A: The pH at equivalence point = 4.88

Q: What are buffers in terms of acid-base equilibria, give an example, and can a buffer capacity be…

A: Buffer solution is a solution that is maintaining it's hydrogen ion concentration pH. With only…

Q: A 21.6 mL sample of 0.350 M dimethylamine, (CH3),NH, is titrated with 0.235 M hydrochloric acid.…

A: Given, the strength of (CH3)2NH - 0.350 Mthe volume of (CH3)2NH - 21.6 mLthe strength of HCl - 0.235…

Q: e molar solubility of Al(C

Q: A 23.1 mL sample of 0.382 M ethylamine, C,H;NH,, is titrated with 0.297 M hydrobromic acid. The pH…

Q: A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH…

A: The pH of the buffer solution is find out using the Henderson-Hasselbalch equation. This equation…

Q: The buffer capacity of a solution is 0.02 .How much(ml) of 1.0 M solution of sodium hydroxide NaOH)…

A: Buffer solution :- A solution which resist the change in its pH value by the addition of small…

Q: er. Calculate the pH of the buffer.

Q: The molar solubility of silver sulfate in a 0.145 M ammonium sulfate solution is М.

A: It is a type of multiple question so I have solved first one for you. If you want to be solved…

Q: A buffer is prepared by adding 115 mL of 0.30 M NH3 to 135 mL of 0.15 M NH4NO3. What is the pH of…

A: A buffer is prepared by adding 115 mL of 0.30 M NH3 to 135 mL of 0.15 M NH4NO3. The pH of the final…

Q: Which of the following statement is incorrect regarding buffer solutions: OBuffer solutions are…

A: Buffer solution : It is a solution formed by weak acid and it's conjugate base pr vice-versa and…

Q: Carbonic acid and sodium bicarbonate act as buffers in the blood. When a small amount of acid is…

A: We know that, our blood normal pH is 7.2 which is act as like buffer because Carbonic acid and…

Q: A 29.5 mL sample of 0.258 M ethylamine, C2H5NH2, is titrated with 0.340 M hydrochloric acid. After…

A: Given- Volume of ethylamine=29.5mL Concentration of ethylamine =0.258M Volume of hydrochloric acid=…

Q: An aqueous solution contalns 0.26 M hypochlorous acid. One Liter of this solutlon could be converted…

A: A buffer solution is an aqueous solution consists of weak acid and it's conjugate base or weak base…

Q: A solution contains 0.230 M sodium hypochlorite and 0.196 M hypochlorous acid. The pH of this…

A: The equation which gives the relationship between pH and pOH of a solution, pK_a and pK_b and ratio…

Q: A solution contains 0.264 M sodium hypochlorite and 0.224 M hypochlorous acid. The pH of this…

Q: An aqueous solution contains 0.34 M ammonium perchlorate. One Liter of this solution could be…

A: The ammonium perchlorate, NH4ClO4, is produced when NH3 and HClO4 are mixed and the aqueous solution…

Q: Which solution has the greatest buffer capacity? Which solution can react with the largest amount…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: A buffer is made by adding 0.300 mol CH3COOH and 0.300 mol CH3COONa to enough water to make 1.000 L…

Q: The maximum amount of calcium sulfide that will dissolve in a 0.161 M ammonium sulfide solution is…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: To 1.00 L of a 0.100 M AgNO3 solution is added an excess of sodium chloride. Then 1.00 L of 0.500 M…

Q: A 26.9 mL sample of 0.282 M ethylamine, C,H5NH,, is titrated with 0.262 M nitric acid. After adding…

Q: Write a balanced chemical equation for the acid-base reaction that would occur if a small amount of…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: A 22.6 mL sample of 0.318 M dimethylamine, (CH3)2NH, is titrated with 0.265 M hydrobromic acid.…

A: First we would write a reaction between given compounds . Then using moles of each compound , we…

Q: A 26.9 mL sample of 0.348 M ethylamine, C2H5NH2, is titrated with 0.391 M hydrobromic acid.…

A: The pH of a solution formed by the mixture of a weak base and its conjugate acid can be calculated…

Q: A 27.4 mL sample of 0.356 M ammonia, NH3, is titrated with 0.279 M hydrobromic acid. At the…

A: Titration curve have three points, 1- Midpoint, 2- Equivalence point and 3- End point In midpoint,…

Q: A 24.9 mL sample of 0.234 M ethylamine, C,H5NH,, is titrated with 0.315 M hydroiodic acid. After…

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, pH of a…

Q: HCl is used to recover oil in oil wells by dissolving rocks, so the oil will flow more easily. In…

A: Given: Percent by mass i.e. %(m/m) of HCl = 10 % And density of solution = 1.073 g/mL.

Q: You could make an acetate buffer by titrating a solution of sodium acetate with ______ to reach the…

A: We want to make acetate buffer. This type of buffer called acidic buffer because it's contain salt (…

Q: A buffer contains equimar amounts of acetic acid and sodium acetate. What is the pH of the buffer?

A: Acetic acid is a weak monoprotic acid

Q: The titration of 50.0mL ot HC2H3O2 (Ka=1.8 x 10-5) 0.100M NAOH. The pH of solution at the Equivalenc…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K2HPO4. Determine the pH change
when 0.061 mol HCIO, is added to 1.00 L of the buffer.
pH change =|
A buffer solution contains 0.229 M CGH;NH3CI and 0.381 M C,H3NH2 (aniline). Determine the
pH change when 0.077 mol HCl is added to 1.00 L of the buffer.
pH after addition – pH before addition = pH change =|
A buffer solution is 0.301 M in HCN and 0.274 M in KCN . If K, for HCN is 4.0×10-10 , what is
the pH of this buffer solution?

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 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

A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of solution. What is the pH of the solution after 0.368 mol of HX is added?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.