The function of a buffer is toO be a strong bazemaintain a neutral pHO change color at the end point of a trationO maintain the pH of a solutionO act as a strong acidD Question 14Which of the following is a buffer system? (Note: NaOH strong base H-CO, weak HC stogacid)0 H₂O and HOOHCO, HƠN HOO NaCl and NaNOOHCl and NaCONSO and NGOH

A buffer solution is an aqueous solution of acid or a base. It consist of a mixture of a weak…

Answered: The function of a buffer is to O be a…

The function of a buffer is to O be a strong baze O maintain a neutral pH O change color at the end point of a nation O maintain the pH of a solution O act as a strong acid

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: 350 mL of a solution with a pH of 1.866? 0.300 g 4.76 mol 0.00927 mol 0.610 g…

A: First calculate molarity and then use molarity formula to get mass.

Q: please highlight the correct answer

A: The hydrogen ions concentration is equal to the concentration of hydroxyl ions in a neutral solution…

Q: What is a buffer? a. a solution that resists change to pH b. any solution at equilibrium c.…

A: Given that : We have to identify which of the following is true for a buffer : a. a solution that…

Q: A neutral solution contains more hydroxide ions than hydrogen ions. True or false

A: Given statement, A neutral solution contains more hydroxide ions than hydrogen ions.

Q: 10.0 mL 0.5 M HCl neutralizes ________ mL 0.1 M NaOH.

Q: che concentrations of H3 O and HCOO¯ in this solution. (K on of H3 Ot M %3D on of HCOO- M %3D

A: Given, Moles of acid = 0.133 mol Volume of solution = 0.442 L Concentration of Acid = 0.133/0.442 =…

Q: The decrease in Molarity of [H*] in an acidic solution will result in O decrease in pH value of the…

A: Explanation to the correct answer is given below

Q: 27. Differentiate acid and base using the Brosted-Lowry definition. *

A: The conjugate acid and base pairs differ only one proton represented as; Conjugate acid ⇌…

Q: What does acid do to marble (calcium carbonate)? What are the generic products of a neutralization…

A: When Calcium carbonate reacts with any acid like HCl or H2SO4 the products formed from the reaction…

Q: Why HCl and NaOH is not a buffer system?

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

Q: The addition of a strong acid like HCI to an aqueous solution would result in O the release of H*…

A: HCl is strong acid . When it is dissolved in water , it will readily release H+ ion in aqueous…

Q: A 0.100 M solution of NH4NO3 has a pH that is More information is needed Equal to 7 More than 7 Less…

A: pH of a solution can be figure out by considering the composition of salt.

Q: 1. A student in the lab places drops of the indicator phenolphthalein a solution. The color of the…

A: a) An indicator phenolphthalein is an acid/base indicator. When phenolphthalein is added to a clear…

Q: Which salt produces a basic solution when dissolved in water? O NANO3 O NaF O NH4CI O FeCl3

A: Answer:- This question is answered by using the simple concept of formation of salts. The salt…

Q: How many mL of 3.2 M KOH(aq) are needed to neutralize 30 mL of 1.6 M HBr(aq)?

Q: In the laboratory a student measures the percent ionization of a 0.559 M solution of hypochlorous…

A: Concentration = C = 0.559 M Percent ionization = % α = 0.0258 % Ka =?

Q: Defermhe the pH of a water fample contang 5 mg/L of fenous iron

A: First Calculate molarity into mol/litre Then use Ph=-log(H+)

Q: Diet coke has a pH of about 2.0, while milk has a pH of about 7.0. The H3O+ ion concentration in…

A: Given, pH of diet coke = 2 pH of milk = 7

Q: A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is…

A: A buffer solution is formed by the dissolution of weak acid and its pH and pKa values should be…

Q: A(n) _____ is a solution characterized by the ability to resist changes in pH when limited amounts…

A: pH is defined as the negative logarithm of the H+ concentration. pH of the acid is less than 7 pH…

Q: What will be the pH of a solution created from a 10-fold dilution of a 0.50 M HNO3 solution? -0.30…

A: The initial concentration of the nitric acid solution is = 0.50 M The pH of 10-fold dilution of a…

Q: A 0.11 M solution of NaOH has a higher pH than a 0.2 M solution of NaOH True or False

A: pH + pOH = 14 So, pH = 14 - pOH pOH = -log[OH-]

Q: TRUE or FALSE 1. pOH is defined as the negative logarithm of the hydronium ion concentration…

A: A question based on concentration terms that is to be accomplished.

Q: 20 The pH of a 0.0085 M solution of HNO3 is

A: Question 20 --> Given - Molarity of HNO3 = 0.0085 M As we know that HNO3 (Nitric acid) is a…

Q: Compared with a solution that has a pH of 6.0, a solution that has a pH of 3.0 contains a) twice as…

A: Given-> pH of solution -1 = 6.0 pH of solution -2 = 3.0

Q: HBr is an Arrhenius acid because A) it produces hydronium ions in solution. B) it produces hydroxide…

A: According to Arrhenius concept, an acid is a substance i.e. when dissolved in water gives H3+ ions.…

Q: The salt NaCl which 100% dissociates is a. Basic b. Neutral c. Not enough information d.…

A: We will first dissociate NaCl in water and the decide its nature.

Q: An acidic solution (select both correct answers): Group of answer choices will turn red-blue litmus…

A: Acidic solution PH between 0 to 7 It contains may H+ ions

Q: What state is the pH indicator (thymol blue) meant for? Gas O Solid O All Liquid Aqueous

A: Thymol blue (thymolsulfonephthalein) is a brownish-green or reddish-brown crystalline powder that is…

Q: If a 0.50 mol/L weak acid is diluted to 0.050 mol/L at constant temperature, which of the following…

A: Given, Initial concentration of weak acid H+ = 0.50 M Diluted concentration of that acid H+ = 0.050…

Q: Which one of the following is a buffer solution?

A: Given question a some acid base compound is given . following compounds is a buffer solution.…

Q: What is pH and how do we control the pH in a sample?

A: Explanation of pH and buffer solutions are described in the step below.

Q: a

A: Dear student I have given answer to your question in the image format.

Q: What is universal indicator?

A: A universal indicator is collectively a mixture of indicators which show a colour change in a…

Q: 1.5 g of limestone are neutralized with 25 ml of 1.00 N HCl. Determine the % calcium carbonate in…

A: 1.00 N HCl is equal to the 1.00 M HCl as HCl is monobasic. Calculate the number of moles of HCl in…

Q: Acid rain the pH of lakes raises lowers maintains neutralizes

A: Acid rain is caused by SO2 and Nitrogen oxided produced by fossil combustion. These acids form low…

Q: 'CI

Q: What does a buffer solution do?* increase the pH neutralizes excess hydrogen and hydroxyl ions…

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

Q: Buffers in the blood are needed to O increase the pH O decrease the pH O maintain a stable pH all of…

A: The human blood contains the buffer solution of carbonic acid H2CO3 to maintain the value of pH in…

Q: A Question 13 (1 point) Retake question *A buffer solution is prepared by adding 6.02 mL of 1.11 M…

A: First, we need to calculate the moles of HI and methylamine in the solution. The number of moles of…

Q: The reaction between an acid and a base is O Endothermic O Exothermic Both endothermic and…

Q: The solution starts off acidic due to the acetic acid present. As more and more sodium hydroxide is…

A: Given Acetic Acid Solution And NaOH basic Solution Acid Base titration performed Condition Given…

Q: Calculate the pH of this solution and determine if the solution is acidic, basic, or neutral

Q: Sulfurous acid, H,SO,, is a weak acid capable of producing two ions. A) What is the pH of a 0.45 M…

A: Answer: Sulfurous acid is a weak acid which will give 2 hydrogen ions on adding in water and an…

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

The function of a buffer is to
O be a strong baze
maintain a neutral pH
O change color at the end point of a tration
O maintain the pH of a solution
O act as a strong acid
D Question 14
Which of the following is a buffer system? (Note: NaOH strong base H-CO, weak HC stog
acid)
0 H₂O and HO
OHCO, HƠN HO
O NaCl and NaNO
OHCl and NaC
ONSO and NGOH

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 3

VIEW

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

Give typed full explanation not a single word hand written otherwise leave it
What change will be caused by the addition of a small amount of the weak base B to a solution containing weak acid HB? pH decrease and [B'] increase no change pH decrease and [B'] decrease pH increase and [B'] increase pH increase and [B'] decrease
When an acid reacts with a base: This is a neutralization reaction Pink color will appear in the resulting solution Both of the answers are correct None of the answers is correct
What is the preferred acid for titrating bases?
What compounds do you add to water to make a buffer?
How do we choose a buffer?
1. Ph HGBr Thf 2. Hzo LATHY excess LiAIHy Hzo
Explain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H,CO, and a salt of its conjugate base NaHCO3 O Excess acid is removed by reacting with NaHCO3; excess base is removed by reacting with H,O O Excess base is removed by reacting with NaHCO3; excess acid is removed by reacting with H2CO3 O Excess H,O is removed by reacting with NaHCO3; excess base is removed by reacting with H,CO
A solution with a pH of 8.5 has a larger hydrogen ion concentration than a solution with a pH of 3.5. True False
QUESTION 7 Match each of the following to the correct definition ◆ Arrhenius Base ◆ Bronsted-Lowry acid Lewis acid A. Acts as a proton acceptor B. Acts as a proton donor C. Acts as an electron acceptor D. Increases the [H*] in an aqueous solution. E. Acts as an electron donor F. Increases [OH-] in an aqueous solution
A solution having a pH of 10 has a larger hydrogen ion concentration than a solution with pH of 2. True False
How many mL of 0.10 M of NaOH must be added to neutralized a 100.0 mL of 0.10 M HF?