Can you please answer these two sub A and B and show all of the steps to the solution acid1131ROCalculate the pH and the concentrations of all speciespresent (H2C3,0.010 M H2CO3 (Kal = 4.3 × 107; Ka2HCO3¯, CO3²-, H3O*, and OH) in%3D%3D79 Calculate the pH and the concentrations of H2SO3,HSO3, SO3², H3O*, and OH in 0.025 M H2SO36.3 × 10 8).(Kal1.5 x 10-2; Ka2 =%3D%3D

Hii there, since there are multiple questions posted. We are answering first question. If you need…

Answered: Calculate the pH and the concentrations…

Calculate the pH and the concentrations of all species present (H2CO3, HCO3¯, CO3²-, H3O*, and OH) in 0.010 M H2CO3 (Ka1 = 4.3 x 107; K2 = 5.6 X 1011). %3D %3D

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 162CWP: For solutions of the same concentration, as acid strength increases, indicate what happens to each...

See similar textbooks

Related questions

Q: Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and…

A: Pure water has an equal concentration of hydrogen ions and hydroxyl ions. The dissociation of water…

Q: Consider the following equilibrium H3 AsO3 (aq) + H2O(1) + → H3O + H2 AsO3 (aq) (ад) Where Ka = 6.0…

Q: The pH of a 0.15-M solution of HSO4− is 1.43. Determine Ka for HSO4− from these data.

A: Given, initial concentration of HSO4− = 0.15 M pH = 1.43 We know that, pH is the negative…

Q: The pH of a solution for which [OH-] = 1.0 x10-6 is %3D

A: pH stands for Hydrogen potentials. pH is a negative logarithm of the concentration of hydrogen ions.…

Q: Calculate the pH of a solution that is 0.0330 M in a. NaH,PO4 (Kal = 7.11 x 10-3, K,2 = 6.32 ×…

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

A: First the equilibrium concentration of H3PO4 is determined.

Q: What is the pH of 0.75 M HC2H302 solution? K.= 1.8 x 105 and Kn=1.00 x 10-14 HC2H3O2 + H2O H3O* +…

Q: Determine the pH level of a solution that has 0.05385 M of Pyridine, given that the Kb of pyridine…

A: Given, Concentration of the Pyridine solution (C) = 0.05385 M Kb for pyridine = 1.620 x 10-6 Note:…

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…

A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid

Q: In the reaction: BCI3 + NH3 The Lewis acid is: (c) B-NH3 1. O cr O H,O O H O NH3 BCly

A: A Lewis acid is a chemical species which has an empty orbital in which it is able to accept…

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: Calculate the pH

Q: Calculate the pH of a 3.12×10-3 M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

Q: Determine [OH–], pOH and pH of a 0.41 M aqueous solution of LiC3H5O3 (K b = 7.1×10-11). [OH–] =…

Q: Calculate the Hydroxide ion Concentration of a Solution of Barium Hydroxide with a pH of 3.3 -11 a.…

A: Given:: pH of Ba(OH)2=3.3 [OH-] = ?

Q: Calculate the pH of a solution with [H3O+] of 2.42×10-5. pH=_____

Q: Which of the following salt aqueous solution has a pH = 7 at 25 °C? %3D O NANO3 O LizSO3 O NH CI O…

A: Answer is NaNO3 NaNO3 salt is of neutral nature. By neutral nature we means, Salt is formed by…

Q: What is the pH of 0.390 M HC1(aq)? O 0.41 0.390 O 13.61 O 13.59 O7.00

A: We have to predict the pH of the solution.

Q: Calculate the pH and in a 0.088-M H2S solution. Assume Ka1 1.0 x 10-7 %3D K2 1.0 x 10-19 %3D pH =…

Q: Calculate the pH of a 0.100M solution of the weak base NH3. Kb of NH3 1.8×10. %3D 3)

Q: Household bleach is prepared by dissolving chlorine in water. Cl2 (g) + H2O « H+ (aq) + Cl-…

A: PHis defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: Determine the pH of a 2.79 M solution of acetic acid (CH3COOH, ka=1.8x10-5)

Q: Calculate the pH of a 0.528 M aqueous solution of benzoic acid (C,H3COOH, K, = 6.3x10). %3D pH =

A: concentration of Benzoic acid (C6H5COOH) = 0.528 M Ka of Benzoic acid = 6.3 x 10−5

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the…

Q: Find the pH of 0.54 M C5H5N(aq) given that its Kb = 1.7×10-9.

Q: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…

A: Given, for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…

Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa). Kb for HCOO− = 5.9 × 10−11

A: Given :- [HCOONa] = 0.31 M Kb for HCOO- = 5.9 × 10−11 To calculate :- pH of solution

Q: [H3O*] [OH]] Acidic or Basic? pH РОН 1.2 x 10-3 4.18 4.2 x 10-11

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Calculate the pH of 0.40 M NH3 solution, Kb = 1.8 x 10° M.

A: Given :- concentration of NH3 solution = 0.40 M kb for NH3 = 1.8 × 10-5 M To be calculated :- pH…

Q: A solution for which [H+] = 1.0 x 10-3 will have a pH of a. 1.00 b. 3.00 c. 5.00 d. -5.00

A: Given information, [H+] = 1.0 x 10-3

Q: c. H20 = Lewis Base (donate 10. Calculate the pH of 0.3M solution of NH,Br if Ka of NH4* = 5.6x10-10…

A: The pH of a 0.3 M solution of NH4Br is to be calculated if Ka of NH4+ = 5.6×10-10

Q: 2. Calculate the pH of a 0.200 M solution of H2SO4. Ka2 for H2SO4 is 1.2 x 102. (Since Kaz is high,…

A: Step -1 we know that PH = -log(H+) H2SO4 - gives two H+ ions in dissociation condition. So, 2 x…

Q: Calculate the pH of a 0.20 M solution of NH4NO3. (Kb(NH3) = 1.8 x 10)

A: Salt of Weak base and Strong acid pH = 7 - 1/2 ( pKb - logC )

Q: Calculate the pH of a 0.01 M NH4(CH3COO) given Kb=1.6E-5 for NH3 and Ka=1.754 E-5 for CH3COOH. A. 7…

A: Ammonium acetate is a salt of weak acid and weak base. The pH of such salts can be expressed as…

Q: How many moles of NH3 must be dissolved in water to give 615.4 mL of solution with a pH of 10.96? K…

A: The number of moles NH3 disolved in water is given below

Q: Determine the [H*]. [OH ]. and pH of a solution with a pOH of 13.48 at 25 °C. [H*] = (OH] = %3D pH =

A: Hi, as you have posted 2 questions and have not mentioned which one you want us to solve, hence we…

Q: Acid Ka HC3HSO3 1.4 x 104 HOCN 3.5 x 104

A: Given acids, Lactic acid - HC3H5O3 Cyanic acid - HOCN

Q: Find the pH of a 0.247 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C. 11.32 2.68…

Q: Determine the pH of 0.25M CH3COONA solution. Kg of CH3COOH = 1.8×105 Select one: 10.08 O 9.08 O 4.90…

A: Sodium acetate is a salt of a weak acid, acetic acid, and strong base, sodium hydroxide. The salt of…

Q: Determine [OH], pOH and pH of a 0.63 M aqueous solution of LIC3H;O3 (K , = 7.1×10-11). [OH]= M РОН 3…

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

Q: Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D 0.120…

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00789 M…

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M solution of…

A: Given : Concentration of (CH3)2NH = 0.103 M And Kb of (CH3)2NH = 5.90 X 10-4 Since (CH3)2NH is a…

Q: Predicting acid or base strength from the conjugate relative pH of 0.1 M aqueous solution species…

A: Answer: In this problem we have to arrange the solution in order of increasing pH.

Q: Calculate the molar concentration of OH− ions in a 0.077 M solution of ethylamine (C2H5NH2;…

A: Given, Concentration of the ethylamine solution (C) = 0.077 M Kb for ethylamine (C2H5NH2) = 6.4x10-4…

Q: A.) What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic…

Q: Calculate the pH of a 0.20M c2h5nh2 solution kb=5.6x10^-4

A: Ethylamine(CH2CH2NH2) is a base (because Ethylamine has one lone pair to accept a proton(H+)).…

Q: For a 9.03x102 M solution of H,CO3, calculate both the pH and the CO, ion concentration. 2- H2CO3 +…

Q: Calcualtw the pH of a 0.217 M HC7H5O2 aqueous solution. Ka for HC7H5O2 is 6.5 x 10^-5.

A: pH of an acid is equal to negative logarithm of concentration of H+ ions.

Question

Can you please answer these two sub A and B and show all of the steps to the solution

acid
1131
ROCalculate the pH and the concentrations of all species
present (H2C3,
0.010 M H2CO3 (Kal = 4.3 × 107; Ka2
HCO3¯, CO3²-, H3O*, and OH) in
%3D
%3D
79 Calculate the pH and the concentrations of H2SO3,
HSO3, SO3², H3O*, and OH in 0.025 M H2SO3
6.3 × 10 8).
(Kal
1.5 x 10-2; Ka2 =
%3D
%3D

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

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 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

Papaverine hydrochloride (abbreviated papH+Cl; molar mass = 378.85 g/mol) is a drug that belongs to a group of medicines called vasodilators, which cause blood vessels to expand, thereby increasing blood flow. This drug is the conjugate acid of the weak base papaverine (abbreviated pap; Kb = 8.33 109 at 35.0C). Calculate the pH of a 30.0-mg/mL aqueous dose of papH+Cl prepared at 35.0C. Kw at 35.0C is 2.1 1014.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Ka
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’