Using the reaction below, predict the effects on sulfuric acid concentration (increase/decrease) if 0.1M sodium bisulfite is added to the solution. Briefly explain. H2SO4(aq) + H2O(l) ⇌ HSO4−(aq) + H3O+(aq)

Using the reaction below, predict the effects on sulfuric acid concentration (increase/decrease) if 0.1M sodium bisulfite is added to the solution. Briefly explain. H2SO4(aq) + H2O(l) ⇌ HSO4−(aq) + H3O+(aq)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 118QRT

See similar textbooks

Related questions

Q: Predict which solution in each of the following pairs will produce the solution of the lowest pH.…

A: pH which historically defines the "potential of hydrogen" is basically a measure of the acidity or…

Q: how many moles of ammonium nitrate would be required to prepare .40 L of solution that is ph 5.40

A: NH3 + HNO3 → NH4NO3 weak base strong acid salt Salt…

Q: 8) A 0.185 M solution of a weak acid has a pH of 2.95. Calculate the acid ionization constant (Ka)…

A: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant Ka…

Q: Cranberries are rich in benzoic acid. Assuming that the only source for hydronium-ions in…

A: The solution is as follows:

Q: Carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.2 x 10-7 and Ka2 = 4.7 x 10-11. Calculate the…

A: It is given that H2CO3 is a diprotic acid, and has Ka1 = 4.2×10-7 and has Ka2 = 4.7×10-11, and the…

Q: 3) into a 1.000 liter volumetric flask, and suddenly realize that you don't have all the reagents…

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

Q: a) A chemist found an old bottle in his chemical store labelled 'monoprotic carboxylic acid, Mr =…

Q: Calculate the equilibrium concentrations of H3O+, Acetate ion, and Acetic acid in a 0.20M Aqueous…

A: The chemical equation and equilibrium equation for the dissociation of acetic acid are shown below.…

Q: Explain how can you prepare pH=4,5,6,7,8,9 HCl solution starting with 5 mL of 10³ M HC1 stock…

A: SOLUTION: Step 1: Preparation of different pH solutions is possible by diluting the stock solution…

Q: Calculate the concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data: Ka1 = 4.2×10-7…

Q: Explain why the observed color change with bromcresol green for each of the four solutions is…

A: Since I am answering the first three sub-parts of multiple sub-parts. Please repost the question and…

Q: Solve the following problems on the pH computation of unbuffered and buffered solutions. Show the…

A: NOTE - As per our company guideline we can answer only 3 sub parts. Kindly repost the question…

Q: Assuming complete dissociation, what is the pH of a 3.25 mg/L Ba(OH), solution?

Q: Solve the following problem, taking turns in your group to explain how to do the next step: What is…

Q: 5. Sodium phosphate, NasPO4, is an ingredient of some preparations used to clean walls before they…

Q: a. Calculate the degree of ionization of 0.25 M HCHO2 (formic acid) solution. K. (formic acid) = 1.7…

A: a) The degree of ionization of 0.25 M HCHO2 is to be calculated. b) The degree of ionization of 0.25…

Q: Saccharin is a monoprotic acid. If the pH of a 6.30 x 10–3 M solution of this acid is 5.63, what is…

A: The dissociation of saccharin is given as, HSac↔H+ + Sac- By definition, the acid dissociation…

Q: Calculate accurately the percent ionization of a 0.010 M solution of nitrous acid (HNO2). Recall…

A: The dissociation of nitrous acid in water is given by

Q: What is the pH of a solution that is 0.125 M in maleic acid, a DIPROTIC acid with Ka1=1.2x10-2 and…

A: Maleic acid dissociates in two steps. The major concentration of hydrogen ion is released in the…

Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

Q: Draw Lewis structures that show how electron pairs moveand bonds form and break in the following…

A: Electron pair acceptor called as Lewis acid and electron pair donar called as Lewis base.

Q: A weak monoprotic acid, HA dissociates by 2.416 % and has a pH of 3.61. Calculate the Ka value for…

A: percent dissociation of HA is 2.416% pH = 3.61

Q: A solution is prepared at 25 °C that is initially 0.14M in propanoic acid (HC,H,CO,), a weak acid…

A: Given :- Concentration of propanoic acid = 0.14 M Concentration of potassium propanoate = 0.012 M…

Q: Calculate the final pH when 2.6 mmol NaOH is added to 1 mmole phosphoric acid, given pka1 = 2.1,…

A: Given, mol of NaOH = 2.6 mmol pKa1=2.1pKa2=7.2pKa3=12.4

Q: An acid is weaker if it presents: i) fewer protons have ii) Lower degree of dissociation iii) Lower…

A: ◆ If the pH of solution is low that means acid is strong. As, we increase the pH of the solution,…

Q: The hydrogen oxalate ion HC,O," is amphoteric. Show how this is so by completing the following…

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

Q: 8. Our bodies are able to preserve a near constant pH due to the presence of hydrogen carbonate…

A: Amphoteric Compounds A compound that acts as acid as well as base is called an amphoteric compound.…

Q: 7. Which of the corresponding salts will produce a basic solution? а. NaHSOA b. КCN c. MgCl2 d.…

A: Identify Salt that makes basic solution in water. As per the Guidelines of the Q&A Platform, I…

Q: What is the approximate pH of a solution prepared by mixing equal volumes of 0.05 M methylamine and…

A: Given - Molarity of methyl amine = 0.05M Molarity of hydrochloric acid = 0.2M n- Volume of Methyl…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

Q: In an experiment, it is found that the pH's of four salts, AA, AB, AC, and AD are 5.0, 6.5, 11.0 and…

A: Given: The pH values of AA, AB, AC and AD are 5.0, 6.5, 11.0 and 9.0 respectively.

Q: in a 0.25 M solution of a weak BOH base, the OH- concentration is 2.4 × 10-³M.What is the…

A: The Question is based on the concept of chemical equilibrium. we have been given a weak base whose…

Q: 6. Brønsted-Lowry definitions can be used to classify substances as acids or bases. a. Define the…

A: 6. a) A Brønsted-Lowry acid is any species that is capable of donating a proton— H+ b) pH is…

Q: Give the formula of the compound which will be dissolved in HNO3? STRONG ACIDS…

A: Solubility

Q: 9. Predict the pH of the resulting solution when we mix 50.0 mL of 0.010 M HClO with 50.0 mL of…

A: We'll answer the first question since the exact one wasn't specified. Please resubmit a new question…

Q: Phenolphthalein reacts to basic solutions (pH above 7) by changing to a pink color. If you had…

A: To turn the solution pink , the pH should be raised to pH = 7 or above.

Q: Suppose you decreased the pH of the biotin solution from 7.0 to 3.0 - what would happen to the…

A: We have to explain the effect of decreasing pH on the structure of the biotin.

Q: EFFECTS OF SALTS ON pH (Lewis Acids and Bases) Determine the effect on the pH when zinc(II) chlorate…

A: When we add an acidic salt to water, the pH of water decreases due to the formation of H+(aq) ions…

Q: 5. What is the approximate ratio of [A]/[HA]ions in a 0.10 M aqueous solution of H2A? Assume that…

Q: The ion HTe− is an amphiprotic species; it can act as either an acid or a base.(a) What is Ka for…

A: a) When HTe− behaves as acid, it deprotone to produce Te2- HTeacid- + H2O ⇌Te2-Conjugate base…

Q: The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At…

Q: Carbonic acid (H;CO:) is widely used in the production of sodas, soft drinks, sparkling wines, and…

A: a.) Carbonic acid is a diprotic acid so it have two acidic protons and hence two ionization…

Q: Which of the following acids is the best to prepare a buffered solution with a pH = 3.50? Justify…

A: A buffer solution is the mixture of a weak acid and its conjugate base in such a way so that…

Q: Which of the following statements correctly describes the hydronium-hydroxide balance in the given…

A: In general, the acid, basic and neutral solutions are defined as: 1) An acid solution is the one in…

Q: Quinine (C20 H24 N2O2) is the most important alkaloid derived from cinchona bark. It is used as an…

A: Given : pKb1 = 5.1 pKb2 = 9.7 Mass of quinine = 1 gm Volume of solution = 1930 ml

Q: Hypobromous acid, HOBr, has an acid dissociation constant of 2.5 × 10–9 at 25°C. What is the pOH of…

A: For a weak acid, we know,[H+] = √(Ka.c)= √ ( 2.5 x 10^-9 x 0.015)= 6.12 x 10^- 6

Q: 12. The pH of 0.15 M butylamine, C4H9NH2 Solution is 12.0 at 298 K. Calculate a. dissociation…

A: Given 0.15 M C4H9NH2 PH= 12 Calculate A) dissociation constant of the base B) degree of…

Q: a) Carbonic acid (H,CO;) is a weak diprotic acid. Write expressions for Kj and K, of H,CO,. Note…

A: The equilibrium equation expression for Ka1 and Ka2 are shown below. Ka1=H+aqHCO3-aqKa2=H+aqCO32-aq…

Q: 4. Which one of the following salts is insoluble in water? а) PЬСОЗ b) Вa(ОН)2 c) Zn(NO3)2 d) NazSO4…

A: 4. Many ionic compounds are soluble in water, but some dissolve only to a small extent; still others…

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

Using the reaction below, predict the effects on sulfuric acid concentration (increase/decrease) if 0.1M sodium bisulfite is added to the solution. Briefly explain.

H₂SO_4(aq) + H₂O_(l) ⇌ HSO₄⁻_(aq)+ H₃O⁺_(aq)

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

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

Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
1. Arrange the following in order of increasing pH of their corresponding solutions. a. CH3NH3Cl, NaCH3COO, RbBr b. K2C2O4, C2H5NH3Br, Ba(ClO4)2 2. Oleic acid (which can be denoted as HOL), is a weak acid. Considering its sodium salt, sodium oleate (NaOL), calculate the pKa of HOL given that a 0.100 M solution of NaOL has a pH of 9.01. (hint: Kw=Ka * Kb).
How is it possible to produce solutions with similar pH values without using acetic acid Explain chemically what is occurring in solution.HC2H3O2 NaC2H3O2 NaOH HCL
The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2
What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5
Write the chemical equation and the Ka expression for theacid dissociation of each of the following acids in aqueoussolution. First show the reaction with H+(aq) as a productand then with the hydronium ion: (a) C6H5COOH,(b) HCO3-.
For a solution that is 0.20 M in oxalic acid (H2C2O4), write the reactions for the ionization of this diprotic acid. The acid ionization constants are Ka1= 6.5 x 10^-2 and Ka2= 6.1 x 10^-5. Calculate the pH, [HC2O4-] and [C2O42-].
Solve the following problems on the pH computation of unbuffered and buffered solutions. Show the complete solution and use the correct number of significant figures. 1. Calculate the [H+], [OH-], pH, pOH of the following unbuffered solution: A) 0.0010M HCl B) 0.0010M NaOH 2. Calculate the [H+], [OH], pH, pOH of the unbuffered solution: A) 0. 01M CH3COOH; Ka = 1.8 x 10 - 5 3. Calculate the pH of the following buffered solution: A buffer solution is made up of 0.90 M formic acid and sodium formate with a Ka 1.8 x 10-4.
The ion HTe− is an amphiprotic species; it can act as either an acid or a base.(a) What is Ka for the acid reaction of HTe− with H2O?(b) What is Kb for the reaction in which HTe− functions as a base in water?(c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe−] in a 0.10 M solution of H2Te.
Calculate the pH of the solution prepared by dissolving 2.675 g of NH4Cl in 250 mL of water. Write the dissociation reactions in water. MNH4Cl: 53,5 g/mol (KNH3)= 1,8x10^-5
What is the pH of a solution that is 0.125 M in maleic acid, a DIPROTIC acid with Ka1=1.2x10-2 and Ka2=4.7x10-7.
7) If NH4OH at 30.0 °C is 1.20 % ionized is 0.250 M solution, what is its ionization constant and the % ionization in 0.500 M solution?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS