Question 36 of 43SubmitCarbonic acid, H,CO3 is a diproticacid with Ka1 = 4.3 × 10-7 and Ka2= 5.6 × 10-11. What is the pH of a0.16 M solution of carbonic acid?134C78+/-x 10 0Tap here or pull up for additional resourcesLO

Answered: Image /qna-images/answer/96ca6b5f-20d1-4b5e-8568-97fdb8bad7f8.jpg

Answered: Carbonic acid, H,CO3 is a diprotic acid…

Carbonic acid, H,CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 x 10-1". What is the pH of a 0.16 M solution of carbonic acid?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.16QAP

See similar textbooks

Related questions

Q: HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.054M in…

Q: Carbonic acid, H2CO: is a diprotic acid with Ka1 = 4.3 x 107 and Ka2 = 5.6 x 10 11. What is the pH…

Q: What is the concentration of a solution of (a) KOH for whichthe pH is 11.89, (b) Ca(OH)2 for which…

A: We know that, the pH of the solution is equal to the negative log10 of the hydrogen ion…

Q: Hydrofluoric acid, HF(aq), is a weak acid with Ka = 3.5 x 10–4. What isthe pH of 0.10 M HF(aq)?

A: Answer :- Acid dissociation constant :- The equilibrium constant for an dissociation of acid is…

Q: Carbonic acid, H2COS is a diprotic acid with Ka1 = 4.3 x 10 7 and Ka2 = 5.6 x 10 11. What is the pH…

A: Answer

Q: The Ka, for propionic acid, HC3H5O2, is 1.30 x 10^ -5. What is the pH of a 0.0850 M propionic acid…

A: The dissociation reaction of propanoic acid is given by HC3H5O2 -----> H+ + C3H5O2- hence Ka = […

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.18 M solution…

Q: Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc) builds up in the blood of persons with…

A: Given data: The pH of Phenylacetic acid = 2.62. The concentration of C6H5CH2COOH [C6H5CH2COOH] =…

Q: If an acid, HA, dissociates to 0.1% when added at a final concentration of 0.05M in water, that is:…

A: 1- First calculate the H3O+ ion concentration : [H3O+] = ( Concentration ) × ( Degree of…

Q: 2. Phenol, CH;OH can act as an acid in an aqueous solution. The Ka of phenolis around 2.1 x 10°, and…

A: pH = -log[H+] pOH = -log[OH] Also, pH + pOH = 14 Also Ka and Kb has a relationship Ka × Kb = Kw

Q: A solution at 25 °C has [OH-] = 6.7 * 10 -3 . What is the pH of the solution?

A: [OH-] = 6.7 × 10-3 Temperature = 25°C pH of the solution = ?

Q: I'm not sure how to solve this.

A: First the equilibrium concentration of H3PO4 is determined.

Q: Carbonic acid, H:COs is a diprotic acid with Ka1 = 4.3 x 10 7 and Ka2 = 5.6 x 10 11 What is the pH…

A: H2CO3 is the weak dibasic acid as it gives two H+ ions. Since, value of Ka1 of H2CO3 is very-very…

Q: Given a diprotic acid, H₂A, with two ionization constants of K₁ = 4.5 x 104 and K = 2.2 x 10-12,…

Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: What is the concentration of a solution of (a) KOH for which the pH is 11.89, (b) Ca(OH)2 for which…

A: We use the PH equation for calculation for H+ concentration. Then apply Ionic product of water to…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

Q: If the Ka of a monoprotic weak acid is 7.8×10−6, what is the pH of a 0.47 M solution of this acid?

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: A solution contains [OH-] = 4.88 x 10-6 M. What is the pH of the solution?

A: Given The concentration of OH- is 4.88×10-6 M.

Q: Calculate the pH of a solution (aq., 25 oC) when 20.00 mL of 0.284 M HNO3 is mixed with 30.00 mL of…

Q: What is the molar concentration of a weak acid [HA], if the ka = 6.34 x 105 and the [H*] = 9.77 x…

A: Dissociation of weak acid : HA ⇌H+ + A-

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: A solution at 25 °C has 3OH-4 = 6.7 * 10-3. What is the pH of the solution?

A: The pOH of a solution is given by, pOH = -log[OH-] The relation between pH and pOH is given by, pH +…

Q: A diprotic acid, H:A, has Ka1 = 3.4 × 104 and Ka2 = 6.7 × 10-°. What is the pH of a 0.17 M solution…

Q: Indicate the pH of the following

A: pH = -log[H+] pH + OH = 14

Q: What is the pH of a 8.1 × 10-6 M KOH solution?

A: The pH scale is introduced by the scientist Sorensen in order to express the [H3O+] ion of a…

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

Q: The pH of a solution at 25°C in which [OH]= 2.0 x 10 is: 1 9.52 4.76 4.69 3.30 9.30

A: In this question, we want to determine the pH of the Solution. You can see details Solution below…

Q: A hypothetical weak base has Kb = 5.0 × 10−8. Calculate the equilibrium concentrations of the base,…

A: Given: Kb for the weak base = 5.0 × 10-8 Concentration of the weak base = 0.15 M We have to…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

Q: If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.19 M solution of this acid?

A: Given, Concentration of monoprotic weak acid = 0.19 M Ka of monoprotic weak acid = 8.3 × 10-6

Q: Which of the following is the strongest acid: н, с. ОА Ов C OD A 'OH H, C FH В OH HC C OH F ж Н D…

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.290 M solution of methylamine?

Q: Carbonic acid, H.CO, is a diprotic acid with Ka1 = 4.3 x 10' and Ka2 = 5.6 x 101". What is the pH of…

A: Carbonic acid (H2CO3) is a diprotic acid because on heating it liberates 2H+ ions. Given: [H2CO3] =…

Q: The Ka for cyanic acid HOCN is 3.5 x 10-4. What is the pH of a 0.37 M solution of the acid? What is…

Q: Calculate the pH of an aqueous solution of 6.45×10-2 M sodium sulfite. pH = ?

A: Sodium sulfite is salt of mixture of strong base sodium hydroxide(NaOH) and weak acid sulfurous…

Q: HClO is a weak acid (Ka=4.0×10−8Ka=4.0×10−8) and so the salt NaClO acts as a weak base. What is the…

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.029M in…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.58 M solution…

A: Since the Ka1 of H2A is >> Ka2 of H2A Hence we can assume only the first dissociation of H2A…

Q: Phosphoric acid, H;PO,(aq), is a triprotic acid, meaning that one molecule of the acid has three…

Q: Lemon juice has a pH of about 2. What [H3O+] is this?

A: Given that the pH of lemon juice is 2. To calculate the concentration of H3O+ ions in the lemon…

Q: What is the pH, pOH and [H3O+] of a 0.022M Sr(OH)2 solution?

Q: What is the pH of a solution with [H3O+] of 1.9 x 10-8 M?

A: Given that, [H3O+] = 1.9×10-8 M pH = ?

Q: Arsenic acid, H3AsO4, is used industrially to manufacture insecticides. Arsenic acid is a polyprotic…

A: Given, Arsenic acid is a polyprotic acid with Ka1 = 2.5 × 10–4 Arsenic acid is a polyprotic acid…

Q: Calculate the pH of a 1.60 M KBRO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10º. 4.25 2.55…

A: ph is the gives the hydrogen ion concentration in the aqueous solution.

Q: Calculate the pH of solutions having the following [H+]: (a) 0.0055 M (b) 1.54 x 10-8 M (c) 3.47…

A: The pH of any solution is given by, => pH = -log[H+ ]

Q: Calculate the pH of a solution made by dissolving 0.0100 mol of NH3 in enough water to give 1.000 L…

Q: Acetic acid (CH3COOH, ?a=1.80×10−5) is a weak acid, so the salt sodium acetate (CH3COONa) acts as a…

Q: HClO is a weak acid (?a=4.0×10−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: An acid is a substance that can furnish the hydrogen ions in the aqueous solution. The weak acid…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

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 2 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

Question 19 In a solution prepared by dissolving 0.100 mole of propanoic acid in enough water to make 1.00 L of solution, the pH is observed to be 2.945. The Ka for propanoic acid (HC3H5O2) is
Morphine (C17H19O3N) (MM 285.34) is a weak base with a kb of 7.4 x 10-7. Calculate the pH of a solution containing a morphine concentration of 1.75 x 10-4 M. C17H19O3N(aq) + H2O (l) = OH- (aq) + C17H19O3NH+ (aq)
Methylamine, CH3NH2, has a Kb of 4.4 x 10-4. What is the pH of a 0.54 M solution of methylamine? Your answer should be to two places past the decimal. Calculate the pH of a 0.21 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).
2,What is the pH of the solution with hydronium ion concentration of 6.3 x 10-12 M? Group of answer choices 10.80 12.60 11.20 11.80 10.20 3,Calculate the pH of 0.50 L of the solution containing 5.61.0g KOH dissolved at 25oC. Group of answer choices 13.30 13.00 0.33 13.70 1.33 4. Calculate the [H3O+]of the solution with pH=9.2. Group of answer choices 2.0 x 10-10 3.6 x 10-9 6.3 x 10-10 9.2 x 10-9 2.0 x 10-9
Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a solution that is 0.00298 M ethylamine.
Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2) solution. The Kb of CH3NH2 is 4.47×10−4.
Ka for formic acid (HCO2H) is 1.8 × 10^-4 . What is Kb for the formate ion (HCO2−)?
Calculate the pH of a solution that is 0.270 M in sodium formate (NaHCO2) and 0.230 M in formic acid (HCO2H). The Ka of formic acid is 1.77 ⋅ 10-4. A) 3.675 B) 13.93 C)10.19 D) 3.815 E)4.952
2. Calculate the pH value of 0.10 M NaH2PO4 solution. Ka1 （ H3PO4 ）= 7.52×10－3; Ka2 （ H3PO4 ） = 6.23×10－8,Ka3（ H3PO4 ） = 4.8×10－13
Can someone help me with the problem below? CH3NH2 is a weak base (Kb=5.0×10−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a solution that is 0.0490 M in CH3NH3NO3 at 25 ∘C?
Calculate the pH of a 0.0261 M trimethylamine hydrochloride solution. Kb ((CH3)3N) = 6.4 × 10−5. Report your answer to TWO places past the decimal.
Calculate the ph of 1.55 M CH3NH2. The Kb for CH3NH2= 4.4 x 10^-4