Answered: What is the pH of a solution with [H^+]…

Science

Chemistry

What is the pH of a solution with [H^+] of: A) 1.7 x 10^-7 M B) 7.5 x 10^-11 M C) 2.45 x 10^-10 M

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 143AE: A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume of water must be added to change...

See similar textbooks

Related questions

Q: What is the pH of a solution that has H+ concentration equal to 5.5 x 10^-5 M?

A: Given Concentration of H+ = 5.5 x 10-5 M

Q: pH of solution with an H3O+ concentration [H_3O^+]= 1.00 x 10^-2 M [H_3O^+]= 5.42 x 10^-12 M

A: pH is termed as the negative logarithm of hydrogen ion concentration. It can be calculated as: pH =…

Q: what is a ph of a solution with [OH^-] of 2.2x10^-7 M

Q: Calculate the pH of a solution if the concentration of H+ is 5.8 x10^(-6) M

A: pH = - log (H+) (H+) = 5.8 × 10-6 M Substituting the concentration of hydrogen ion in above…

Q: solution contains [H+] = 0.0034 M a) What is the pH of the solution? pH…

A: Given, Hydrogen concentration = [H+] = 0.0034 M We need to calculate the pH of the solution using…

Q: Calculate the pH of each solution.(a) [H3O+] = 1.7 * 10-8 M(b) [H3O+] = 1.0 * 10-7 M(c) [H3O+] = 2.2…

Q: Calculate the pH for the solutions which have the following [H3O+]. 9.5 x 10^-6 7.9 x 10^-3 4.4 x…

A: pH for the given [H3O+] concentrations has to be calculated.

Q: what is the pH of a bleach solution that has a [OH-]=1.9x10^-3 M? Is the bleach acidic,basic or…

Q: What is the pH of a solution which is 0.023 M in weak base and 0.035 M in the conjugate weak acid…

A: The solution is as follows:

Q: 12) The pH of a solution is measured to be 10.40. What are the values of [H3O+] and [OH-] for this…

A: The pH of the solution = 10.40 H3O+=?OH-=?

Q: Q2: Calculate the pH of a 1.3 * 10 ^ - 9 M HBr solution ?

Q: what is the pH of a solution that is 1.45 x 10^-3M H3O+

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

Q: In converting from the pH of a solution to the corresponding H3O+ concentration, the following…

A: The answer of the given question is given below

Q: A sample of fresh pressed apple juice has an [H*] = 1.7 x 104 M Calculate the pH of this apple…

Q: Find the pH of a solution that is 9.0x10^-2 M in H2CO3

A: To calculate the pH we have to know the concentration of [H3O+]. As we know pH= -log [H3O+] in the…

Q: What is the pH of a solution that has [OH–] = 6.92x10-11 M.

Q: he pH of a half-neutralized solution is 1.86. What is the value of [H+] and Ka?

Q: Calculate pH and pOH of a solution with [OH-] = 5.92×10-8 M

A: Given [ OH- ] = 5.92 × 10-8 M PH = ? POH = ?

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

Q: The pH of a solution with [H3O+] = 1.0 × 10−3 M is: A) –3.00 B) 3.00 C) 11.00 D) –11.00 E) 1.00…

Q: 1) Write a chemical reaction to show the neutralization of hydriodic acid (HI) by sodium hydroxide…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

A: pH is equal to the negative logarithm of hydronium while pOH is equal to the negative logarithm of…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 8.97? (b) What are [H₃O⁺], [OH⁻],…

A: The concentration of the hydrogen ions in the solution is determined in the pH scale.…

Q: Determine the H30* concentration in the following solutions. Identify each solution as acidic,…

A: If the pH>7: Basic solution If pH < 7: Acidic solution If pH =7: Neutral solution (a) pH…

Q: What is the [OH-] for a solution with a pH of 1.68? a) 2.1 x 10-2 mol/L b) 2.09 x 10-2 mol/L c)…

A: Given a solution with a pH of 1.68 we are asked to calculate the concentration of hydroxide ion…

Q: what is the pH of a solution with [OH-] = 2.93×10^-9M

A: Given, [OH-]=2.93×10-9 Mwe are asked to calculate the pH of solution.

Q: 4) Calculate the [H+] in a solution with a pH of 9.88? a) 4.1 M b) 9.9 M c) 7.6 x 10^-5 M d) 1.3…

A: pH of the solution is 9.88

Q: What's the pH of a solution with an H+ concentration of: 1.247 x 101º. Round to 2 decimal places.

A: pH measures how the solution is basic or acidic lower the pH value the solution will be more acidic…

Q: What is the pH of a 5.3 x 10^-6 M HBr solution?

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

Q: [H+] of a solution

Q: What is the pH of a bleach solution that has a [OH-| = 2.4 x 10-5 M? pH = Is bleach acidic, basic,…

Q: What is the pH of a 8.7x10^-3 M HI solution

A: given : [HI] = 8.7 × 10-3 M to calculate :- pH of solution

Q: The pH of a solution that has measured (H+) of 6.8*10^-9 M is

A: We have given that [H+] = 6.8×10-9M pH is measure the acidity and basicity of aqueous…

Q: Calculate the pH of a solution with [H+]= 1×10−4 M .

A: The pH of a solution is calculated by using the hydrogen ion concentration by using the following…

Q: What is the pH of a 1.7 x 10^-3 M HI solution?

A: pH is a measure of acidity and basicity of solution. When pH value is below 7 solution is acidic.…

Q: How can you increase the pH of a solution when The pH of its equal 7 ? O (a) By adding a small…

A: The negative logarithm of hydrogen ion concentration is defined as the pH of the solution. It is…

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

What is the pH of a solution with [H^+] of: A) 1.7 x 10^-7 M B) 7.5 x 10^-11 M C) 2.45 x 10^-10 M

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

Step 2

Step 3

Step 4

Step by step

Solved in 4 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

A solution of baking soda, NaHCO3, has a pH of 10.08. What is the percent (by mass) of NaHCO3 in a 235-mL solution? (Assume a density of 1.00 g/mL.)
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
Calculate the pH of each of the following solutions. a. 0.10 M CH3NH3Cl b. 0.050 M NaCN
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume of water must be added to change the pH to 4.000?
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2
At 25 C, a 0.10% aqueous solution of adipic acid, C5H9O2COOH, has a pH of 3.2. A saturated solution of the acid, which contains 1.44 g acid per 100. mL of solution, has a pH = 2.7. Calculate the percent dissociation of adipic acid in each solution.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. HC3H3O3 b. HCN c. H2SO4 d. H2SO3
8-13 Define (a) an Arrhenius acid and (b) an Arrhenius base.
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.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.