Answered: complete the table below: (show your…

Science

Chemistry

complete the table below: (show your solution - given, required, solution, answer) [H+] pH pOH [OH-] 4.84

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

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: Calculate [OH-] in a solution with [H3O+] = 1.5 * 10-4 M.

A: • The values provided in the question are:- i) Hydronium ion concentration of a solution,…

Q: Which of the following is an acid that will dissociate completely in water? × OHF NH3 HCI CH3COOH

A: FOR ANY QUERIES, PING ME HAPPY LEARNING

Q: 1. What is the pH of 6.14×10-³ M HI? Is the solution neutral, acidic, or basic? 2. What is the pOH…

A: (a) Given : [ HI ] = 6.14x10-3 M Required: pH = ? Solution: HI is a strong acid and gets…

Q: Calculate the pH of the following substances a) 057 M HCl b) [H+] = 0.082M c) 250 ml of 0.005…

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

Q: The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution…

Q: Complete the following table. (All solutions are at 25 degrees Celsius) (H3O+) (OH-) pH Acidic or…

A: Complete the following table by using pH rule of acidity and basicity --

Q: Benzoic acid is a weak acid that has antimicrobial properties. Its sodium salt, sodium benzoate, is…

A: Given : pKa of benzoic acid dissociation reaction = 4.2 And initial concentration of benzoic acid…

Q: Measurements of a solution found that the [H+] (aq)] < [OH- (aq)], therefore the solution is (1)…

A: pH of solution is defined as the concentration of hydronium ion H3O+in the solution pOH of solution…

Q: Part 1 Calculate the pH of a solution in which (HO) = 4.26x103 M. Give your answer to two places…

A: Use relation Ph=-log(H+) Ph+poh=14 M1V1=M2V2

Q: How do you find H3O+ from molarity, pH or pOH/OH-?

A: pH = - log [H3O+] pOH = - log [OH-] pH + pOH = 14 [H3O+] = 10-pH [OH-] = 10-pOH [H3O+] [OH-]…

Q: Calculate the [H*] of a solution at 25°C, if [OH-] = 6.1 x 10-11 M. (answer in scientific notation)…

Q: The pH of a basic solution is 10.33. What is [H]?

A: Given details, The pH of the base solution [OH-] = 10.33 To calculate the [H+].

Q: Given a solution in which the pH = 4, determine [H+], [OH-] and pOH.

A: Inorganic chemistry.

Q: The pOH of a basic solution is 5.09. What is [H⁺]?

A: pH is equal to negative logarithmic value of hydrogen ions concentration

Q: What is the [H3O+] in a solution with [OH-] = 2.5x10^-2 M

A: [H3O+] and [H+] represents the concentration of H+ only. We know; [H+] [OH-] = 10-14 [H+] (2.5 ×…

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

Q: The [OH-] = 5.4 x 10-5 M for the NH3 and NH4Cl solution. What is the pH of the solution? pH = [?]

Q: Determine both the H and the pH in a 0.0541 M solution of HNO3 at 25 °C? H= Type your answer here…

A: The concentration of HNO3 solution = 0.0541 M HNO3 → H+ + NO3− The concentration of H+, [H+] =…

Q: What are [H3O+], [OH−], and pH in a solution with a pOH of 10.10? Make sure your answers are given…

A: given, pOH= 10.10

Q: Determine the [OH]- concentration of a solution that has a pH = 4.33 at 25°C?

Q: Determine [OH-] in a solution where [Ba(OH)2] = 0.0249 M.

A: Strong Base - A base which completely dissociates into it's ions in aqueous solution called strong…

Q: In order for a solution to be basic: O H30] = [OH] O H30*] > [OH] O (H3ot] < [OH]

A: Relation for basic solution---

Q: The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's…

A: pH is defined as negative logarithm of hydrogen ion concentration pH= -log[H+] If pH<7 then the…

Q: Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the pOH of the solution. Is the…

A: [OH–] = 8.4 x 10–11 M( Given ) So, pOH = – log [OH–] = – log( 8.4 x 10–11 ) = 10.075 Now, As we…

Q: 54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify…

A: Since, you have given multiple subparts, we will solve the first 3 subparts for you. For other parts…

Q: Aspirin, which is acetylsalicylic acid, was the first NSAID use to alleviate pain and fever. If a…

Q: Calculate the pH of an aqueous solution where the [OH-] is 6.9 × 10^-9 M.

Q: A 4.28⋅10^−2 M solution of HBr is made. (answer each part) part A: What is the pH of this solution?…

Q: 1.If the concentration of OH- ions in an aqueous solution is 1.4 × 10-5 M. a) Find the…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: What is the pH of a solution that has an [OH-] of a 7.3 x 10^-9 M?

A: Given, Concentration of the OH- ion = [OH-] = 7.3 x 10-9 M pH of the solution = ? The formula used…

Q: Determine the [OH'], [H;O*], pOH and pH of a 0.001 M KOH solution.

A: KOH ----> K+ + OH- [OH-] = [KOH] = 0.001 M [ H3O+ ] = Kw÷ [ OH- ] = 10-14/0.001 =…

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 pH of an HF solution of each of the following concentrations. In which cases can you…

A: (a)ICE table for the reaction is given below.

Q: Rank the strengths of phosphoric acid, sulfuric acid and perchloric acid based on their structure.…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: (a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 9.85? (b) What are [H₃O⁺], [OH⁻],…

A: a) pH of a solution is equal to negative logarithm of hydronium ion concentration present in it. So;…

Q: ion The hydroxide concentration in a solution of NaOH is 9.3 x 10¹ M at 25 °C. What is the pH of…

A: Answer:- This question is answered by using the simple concept of calculation of pH . Firstly using…

Q: 6. A substance has a [H,O'] of 5.21 x 10³, determine [OH], pH and pOH and determine if the substance…

A: [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] pOH = -log[OH-] pH < 7 , acidic pH > 7 , basic pH = 7,…

Q: The [?3?+] of a solution is 1.3 ? 10−5, Calculate the [??−], pH and pOH of the solution. Is the…

A: The concentration of H3O+ and the concentration of OH- in a solution are related to each other. The…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Acid Strong or WeakH3PO4…

Q: Calculate [OH-] for each solution. pOH = 13.28 pH = 1.82 pOH =

A: The question is based on the concept of hydronium ion and hydroxide Ion concentration. We have to…

Q: Idendify ALL of the the TRUE statements (there may be more than 1) A) NH4^(1+) and OH^(1-) form a…

A: Arrhenius acid and base has the tendency to lose proton and hydroxide ion respectively. Lewis acid…

Q: A 0.048g sample of solid calcium hydroxide is dissolved in water to form a 750.0ml solution.…

A: PH =- log [H+] POH =- log [OH-] Where [H+] and [OH-] are the concentration of H+ and OH- Molar…

Q: Complete the following table with the needed [H3O*], [OH'], pH, and pOH. Then, classify the solution…

A: We know that the concentration of hydromium ion and hydroxide ion are same in the solution. We also…

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

complete the table below: (show your solution - given, required, solution, answer)

[H^+]	pH	pOH	[OH^-]
		4.84

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

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.
2. The cyanide ion, CN−, accepts a proton from water to form HCN. Is CN− a Bronsted acid or base or is it amphiprotic? acid base amphiprotic
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
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
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
You are asked for the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a strong base, can we say there is no H+. since having H+ would imply that the solution is acidic?
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate (c) KOH (d) Ammonia (e) Water
Which of the following substances are acids in terms of the Arrhenius concept? Which are bases? Show the acid or base character by using chemical equations. a P4O10 b Na2O c N2H4 d H2Te
12.63 For each of the following reactions, indicate the Bronsted-Lowrv acids and bases. What are the conjugate acid-base pairs? CN’(aq) + H2O(€) «=* HCN(aq) + OH’(aq) HCO}-(aq) + H,o+(aq) +* H2CO,(aq) + H,O(€) (C) CH,CtX)H(aq) + HS~(aq)i=i CH}COO"(aq) + H2S(aq)
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.