Answered: The pH of a 0.25 M aqueous solution of…

The pH of a 0.25 M aqueous solution of HF at 25°C is 2.03. What is the value of Ka for HF? 3.7 x 10-2 2.4 x 10-1 9.3 x 10-3 3.5 x 10-4

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: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: Which of the following 1 M solutions would have an acidic pH? Weak Weak Ка Acid Base HCN 4.9 x 10-10…

Q: What is the percent ionization of a 0.1 M monoprotic ?acid solution (Ka = 1.6 × 10-4) at 25°C 0.38%…

A: Given : Ka = 1.6 x 10-4 Concentration (C) = 0.1 M

Q: What is the [H] of an aqueous solution with a pH of 6.2? 3.2 x 10-5 M 6.2 x 10-6 M 6.3 x 10-7 M 1.6x…

Q: Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 8.32. O 5.7 O 8.3 x…

A: pOH of an aqueous solution is 8.32 .We have to calculate the molarity of hydroxide ion in the…

Q: Calculate [H+] for a 3.00×10-4 M aqueous solution of cinnamic acid (HC9H7O2; Ka = 3.70×10-5)

A: The acid (say HA) dissociates in water to produce corresponding ion and hydronium ions. HA…

Q: what is the pH of a solution containing a H+ concentration of 5.2 x 10-9 M

A: The objective of this question is to calculate the pH of a solution given the concentration of H+…

Q: What is the hydroxide ion (OH)concentration of a 0.0325-M solution of ammonia, a weak base with a Kp…

A: We have 0.0325 M solution of ammonia with Kb as 1.76*10-5 . We have to calculate the hydroxide ion…

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

Q: Find the pH and percent ionization of each HF solution (Ka = 6.8 ́ 10-4). In which cases can you not…

Q: Complete the table. That is, fill in any missing entries in the second and third columns. Round your…

A: We know that pH formula given pH = - log [H3O+] Here [ H3O+] = concentration of H+ ion in solution…

Q: At 50°C the value of K w is 5.5 x 1014. A basic solution at 50°C has

Q: What is Ka for a weak monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28 at 25°C? O…

A: To find Ka value of a weak acid, first find out hydronium ion concentration and from that find out…

Q: What is the pH of a solution containing 100 mg/L acetic acid (CH3COOH)? (Ka=1.8x10-5)

Q: For the diprotic weak acid H₂A, K₁1 = 3.5 x 10-6 and K₁2 = 8.3 × 10-⁹. What is the pH of a 0.0500 M…

Q: For the diprotic weak acid H2A, Kal = 3.5 x 10-6 and Ka2 = 7.7 x 10-9. What is the pH of a 0.0400 M…

A: Ka1>> Ka2 it means second dissociation is very small

Q: 0.25 — X X X x = 5.8 х 10-2 pH = [ ? ]

Q: A solution of a weak acid contains 5 mM conjugate acid (HA), 2.5 mM conjugate base (A-), and 2.5 mM…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: What is the [H+] in a solution with a pH of 3.75? Group of answer choices 5.6 x 103 7.5 x…

Q: Fill in each blank cell with the correct value pH [H*] (mol/L) POH 11.7 5.1 x 10-5 2.3 12.2 [OH-]…

Q: Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00. O O 11.00 3.0…

A: pH = -log[H+] pOH = -log[OH-]-> pH < 7 , it is acidic and [H+] > [OH-]-> pH > 7 ,it…

Q: The base protonation constant K of ammonia (NH3) is 1.8 × 10 Calculate the pH of a 1.2 M solution of…

Q: name hypochlorous acid acetic acid 0.1 M KCIO acid solution 0.1 M HONH3Br 0.1 M NaCH3CO₂ 0.1 M KBr…

A: As we know, salt of strong acid and strong base are neutral in nature . salt of weak acid and…

Q: Calculate the pH of 0.30 M NaOH solution ? Kw = 1.0 x 10-14

A: pH is defined as the concentration of hydronium ion in the solution

Q: What is the hydroxide ion concentration of a solution with a pH = 5.50 at 25 °C? %3D

A: pH = 5.50 We know at 25°C; pH + pOH = 14 5.50 + pOH = 14 pOH = 14 - 5.50 pOH = 8.5 Now, pOH = - log…

Q: The pH after adding 23.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is 0.080 1.1 1.4 0.042

A: According to guidelines i can answer only first question, please repost the other question

Q: What is the pH of 0.18 M sodium acetate solution? (Ka = 1, 8x10-5)

Q: Calculate the pH of a solution that is 0.54 M HF and 1.00 M KF. Ka = 7.2x104 pH =

A: Given, Concentration of HF = 0.54 M Concentration of KF = 1.00 M Ka for HF = 7.2 x 10-4 PH = ?

Q: A 1.0 × 10 -2 M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of? 12.30 12.00 2.0 ×…

A: Answer:- This question is answered by using the simp[le concept of calculation of pH of the solution…

Q: 7) What is the pH of a solution prepared by dissolving 0.399 g of NaOH(s) in 8.50 L of water? (Kw…

A: First we need to calculate the concentration of NaOH and OH- using mass and volume. As mole ratio…

Q: Arrange the following solution from lowest pH to highest pH: 0.75 M CH3COOH (K, = 1.8 x 10-5) 0.01 M…

Q: The Ka of acetic acid (HC2H302) is 1.8 x 10-5. What is the pOH at 25.0 °C of an aqueous solution…

Q: A 0.025 M solution of iodic acid, HIO3, has a pH of 1.65. What is the hydronium ion concentration in…

Q: Find the percent ionization of a 0.124 M weak acid solution whose KA = 2.7 × 10–6. Group of…

A: Concentration of Acid (M) = 0.124M Also, Dissociation constant of acid KA=2.7×10-6

Q: What is the pH of a 2.0 L-solution which contains 2.0 x 10-5 moles of H3O+ ions? O - 4.70 4.40 4.70…

A: The pH of a solution is = 5.00 ----> option(d)Explanation:Step 1: Calculation of H3O+ ions…

Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4 The dissociation…

Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. O 4.3 x 10-4 8.6 x 10-6 O 4.9 x…

A: The problem is asking us to find the Ka (acid dissociation constant) of an acid. We are given the…

Q: What is the percent dissociation of a weak acid with pH of 2.59 ? ka = 6.5 × 10-5. 0.50% 2.5% 1.5%…

A: Given values-> pH = 2.59 Ka = 6.5×10^-5

Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

Q: What is the percent ionization of a 0.15 M solution of weak acid that has a pH of 1.86?

Q: Benzoic acid, C6H5COOH, has a Ka = 6.3 x 10-5, What is the percent ionized in a 0.95 M solution of…

A: Final answer is given in explanation please see from there.Explanation:Approach to solving the…

Q: The acid dissociation constants for phosphoric acid (H₂PO4) are Kai = 0.00711, Ka2 = 6.32 x 10-8,…

A: Given data : Ka1 = 0.00711 Ka2 = 6.32×10-8 Ka3 = 7.1×1-13

Q: Calculate the [H₂O+] of a milk of magnesia solution that contains [OH-] = 4.81 x 10-5 M. 1 4 7 +/- 2…

A: The product of the concentrations of ions [H3O+] & [OH-] is always equal to 1.0×10-14 at…

Q: Arrange the following solution from lowest pH to highest pH: 0.20 M CH,COOH (Ka 1.8 x 10-5), 0.20 M…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: What is the pH of a solution that is 0.053 Min HA and also 0.063 Min NaA? (Ka = 4.1 × 10-6) 5.46 O…

A: Henderson Hasselbalch equation, pH = pKa + log [salt]/[acid]

Q: What is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? %3D

A: Answer: ICE table for the dissociation of weak monoprotic acid is shown below:

Q: The pH of a 0.22 M aqueous solution of a weak acid at 25.0 °C is 4.50. What is the value of Ka for…

A: Weak acid dissociated feabily in aqueous solution

Q: For the following reaction, write how the each of the changes will affect the indicated quantity,…

A: According to Le-chatelier's principle when any disturbance is made on equilibrium then it shifts in…

Question

The pH of a 0.25 M aqueous solution of HF at 25°C is 2.03. What is the value of K_a for HF?

3.7 x 10^-2

2.4 x 10^-1

9.3 x 10^-3

3.5 x 10^-4

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

SEE SOLUTION Check out a sample Q&A here

Similar questions

Consider the following data on some weak acids and weak bases: Ka formula HNO₂ 4.5 x 104 -4 hydrocyanic acid HCN 4.9×10 10 acid name nitrous acid solution 0.1 M NaCN Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a 2¹ next to the solution that will have the next lowest pH, and so on. 0.1 M CH₂NHBr 0.1 M Nat 0.1 MC₂H₂NH₂Cl pH choose one 1 (lowest) 4 (highest) choose one base name K₂ formula pyridine CH₂N 1.7 x 10⁹ ethylamine C₂H₂NH₂ 6.4x104
None
Calculate the pH and fraction of dissociation (a) for each of the acetic acid (CH COOH, pka = 4.756) solutions. A 0.00333 M solution of CH, COOH. A 2.15 x 10-12 M solution of CH, COOH. pH = 1 228 X10-7
Each row of the table below describes an agueous solution at about 25 °C. [H,0 ]to Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for to 2 significant digits, and your entries for pH to 2 decimal places. [x,0] solution pH 5.6 x 10 -9 mol/L A O mol/L 7.15 B 0.049 mol/L
The Ka of acetic acid (HC2H3O2) is 1.8 × 10-5 . What is the pOH at 25.0 °C of an aqueous solution that is 0.100 M in acetic acid? choice 1.75 2.87 8.32 11.13 12.06
What is the pH of a solution containing 0.10 M cyanide ion, CN1-? CN1- + H2O < === > HCN + OH1- Kb of CN1- ion = 1.6 x 10-5
What is the pOH of a 0.50 M solution of polyprotic acid H3X with K1 = 2.5 x 10-4, K2 = 5.6 x 10-8, and K3 = 3.0 x 10-13?
What is the K w of pure water at 70.0°C, if the pH is 6.650? 5.02 x 10 -14 1.00 x 10 -14 5.50 x 10 -14 2.24 x 10 -14 2.24 x 10 -7
= O ACIDS AND BASES Making qualitative estimates of pH change Each row of the table below describes an aqueous solution at 25 °C. ? The second column of the table shows the initial components of the solution. Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B C D H₂O, HCIO4 H₂O H₂O, HCIO4 Explanation H₂O Check initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add NaOH add KOH add Na C104 add KI effect of change on pH (check one) X 10 0 С pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same S #tv MacBook Air
Calculate the pH of a 0.859 M NaF solution. Assume Ka(HF) = 1.0 x 10-4
Calculate the pH of a solution that is 0.66 M HF and 1.00 M KF. к, 3 7.2 х 10-4 pH =
What Is the pH of a solutlon of 3.7 M HBr? A -0.651 B) -0.748 0.568 D) -0.568 E 0.748