a Solution 1 has [H]=7.3x10 M, and solution 2 has [H]=6.2x10° M.Calculate pH of both solutions.pH of solution 1 =pH of solution 2 =SubmitSubmit AnswerTry Another Version5 item attempts remaining76°F Watch

pH :- The negative logarithm to the base 10 of H+ ion concentration expressed in mol/L of an…

Answered: a Solution 1 has [H]=7.3x102 M, and…

a Solution 1 has [H]=7.3x102 M, and solution 2 has [H]= 6.2x10 M. Calculate pH of both solutions. pH of solution 1 = pH of solution 2 = %3D

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: What concentration of potassium hydroxide is needed to give an aqueous solution with a pH of 9.770?…

A: pH = 9.770 pH + pOH = 149.770 + pOH = 14pOH = 14 - 9.770pOH = 4.230 pOH = - log [OH-]4.230 = -…

Q: Calculate the pH of each of the following solutions. Ka(НС2 Н3О2) %3D 1.8 х 10 5 Ка(НCN) — 6.2 х 10…

A: #(a): KC2H3O2(aq) is a conjugate base of HC2H3O2(aq). Hence it will undergo hydrolysis to form…

Q: What is the pH of a solution that has [H3O*]= 4.5x10-³ M?

Q: Consider two solutions: solution X has a pH of 5; solution Y has a pH of 7. From this information,…

Q: In a dilute sodium bicarbonate solution, [H] = 1.8 x 10-8 M. Without using a calculator, what…

Q: The equivalence point is reached when a solution is neutralized. OTrue O False

A: This question can be solved by considering the case of acid-base titration, in which a definite…

Q: Rank the following from most to least acidic

A: On the basis of pH, Less the pH more the acidity of compound and vice versa

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid hydrocyanic…

Q: Basic solutions change the color of litmus paper from blue to red. CH3COOH ionizes completely in…

A: 1. This statement is false as base changes red litmus to blue. 2. This statement is false as Acetic…

Q: alculate the pH of the following solutions. a) [H3O*] = 1.0×10-4 M pH=| b) [H;O*] = 0.10 M pH = «)…

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: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: 0-7 = acidic 7-14= basic 7 = neutral

Q: Determine the pH of water solutions with the following characteristics. Classify each solution as…

Q: 16.88 HA and HB are both weak acids although HB is the stronger of the two. Will it take more volume…

A: Given, HA and HB both are weak acids, but HB is stronger than HA. Concentration of NaOH = 0.10 M…

Q: i. 200 mL of a 0.200 M solution Disodium phosphate (Na,HPO) to which 60 mL of 1.0 M HCI is added. pH…

A: Answer: pH of a solution is equal to the negative of logarithm of its hydrogen ion concentration.

Q: Calculate [OH -] and pH for each of the following solutions. (a) 0.0036 M RbOH [OH-] = M pH =…

Q: You want to make up 2.90 L of aqueous hydrochloric acid, HC1(aq), that has a pH of 2.00. How many…

A: Since HCl is a strong acid hence it will dissociate completely into H+ ion Hence concentration of…

Q: Part A [H3O+]=4.7 x 10-8 M Express your answer using two decimal places. pH = pH = [H3O+]=3.0 x 10-³…

A: pH : pH can be defined as the negative logarithm of H+ ion or H3O+ ion concentration pH = -log[H3O+]…

Q: Complete the following table. Each row refers to a single solution. [H'] [OH] pH pOH Acid, Base,…

A: We can fill the table by using following formulas. pH = - log[H+] pOH = -log [OH-1 ] Also pH =…

Q: Write the overall reaction between aqueous HCl and solid NaHCO3 to form sodium chloride, water, and…

A: Since HCl is an acid and NaHCO3 is a base, they undergo neutralization reaction to form sodium…

Q: Calculate the pH of pure water

A: Given :- Kw = 2.4 × 10-14 To calculate :- pH of pure water at 37°C

Q: K.(HC,H3O2) = 1.8 x 10-5 K. (HOCI) = 3.5 x 10-8 K, (NH3) = 1.8 x 10-5 a. 0.2 М КС2НЗ О2 pH = b. 0.33…

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Given, Based on pH scale we can classify type of solution as acidic, basic or neutral. If pH of a…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: Identify each of the following as an acid or a base in terms of the Arrhenius concept. Show the acid…

A: Answer: According to Arrhenius concept, any compound that furnishes hydronium ion in water can be…

Q: When answering this problem, report the answer with the appropriate number of significant figures…

Q: QUESTION 6 If an aqueous solution has a hydronium ion concentration of B.2 x 10* M, (a) what is the…

Q: What is the pH of a solution of 0.35 M Hydrochloric Acid? 60 35 68 7 45 61 75 90 80

A: HCl -------> H+ + Cl- [HCl] =0.35 M pH = -log [H+]

Q: 2. You are given three solutions: HCI (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution…

A: Concept: If pH less than 7 is Acidic solution pH more than 7 is the Basic solution pH= 7 is neutral…

Q: Determine the [H*],[OH-], and pOH of a solution with a pH of 11.63 at 25 °C. [H*] = M [OH-] = M %3D…

A: Since at 25 oC [H+] * [OH-] = 10-14 pH = -log[H+] pOH = -log[OH-] pH + pOH = 14

Q: The pH readings for wines vary from 2.7 to 3.7. Find the corresponding range of hydrogen ion…

A: we have to determine the range of hydrogen ion concentrations for given pH range

Q: A chemist dissolves 158. mg of pure potassium hydroxide in enough water to make up 130. mL of…

A: To find pH, the first step is to find the molarity of KOH solution and then calculate pOH from the…

Q: A solution is made by dissolving 18.7 g of CH₃NH₃NO₃ in 500.0 mL of water. Determine the pH of the…

A: Mass of CH₃NH₃NO₃ = 18.7 g Volume of water = 500.0 mL = 0.500 L pH of solution = ?

Q: You have 1.00 L of a 1.00 M CH3NH₂ solution. You add 0.38 moles of HNO3 to your solution and mix…

Q: 2. A solution of NaCN has a pH of 9.20. Find the [H*] in the solution. Is the solution acidic or…

A: The question is based on the concept of pH of the solution. It is defined as a negative logarithm…

Q: Nicotinic acid, HCGH4NO2, is a B vitamin. It is also a weak acid with K, = 1.4 x 10-5. Calculate…

A: Given : Concentration of HC6H4NO2 = 0.034 M And Ka of HC6H4NO2 = 1.4 X 10-5 Since HC6H4NO2 is a…

Q: Ка (НCN) — 6.2 x 10-10 Къ (NH3) — 1.8х 10-5 0.2 М КС:НзО pH = 0.51 M NaCN pH = 0.4 M NH4C1 pH =

A: pKa = -log(Ka) pKa(HC2H3O2) = 4.74 pKa(HCN) = 9.21 pKb(NH3) = 4.74 A) 0.2 M KC2H3O2 It's sat of…

Q: What is the pOH of (3.03x10^-1) M LİOH? Enter your answer in scientific notation with 3 sig figs. Do…

A: pOH is negative logarithm of concentration of OH- ions. LiOH is a strong base. So, it dissociates…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0114 M solution. The pH of the…

Q: Consider an aqueous solution of Ba(OH)2. If the pH of this solution is pH = 9.47, what is the…

Q: What is the pH of an aqueous solution with [H3O+] = 2×10−14 M? Express the pH numerically using one…

A: Hydronium ion concentration is an important parameter of an aqueous solution. The concentration of…

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

a Solution 1 has [H]=7.3x10 M, and solution 2 has [H]=6.2x10° M.
Calculate pH of both solutions.
pH of solution 1 =
pH of solution 2 =
Submit
Submit Answer
Try Another Version
5 item attempts remaining
76°F Watch

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 3

VIEW

Step by step

Solved in 3 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

For many weak acid or weak base calculations, you can use a simplifying assumption to avoid solving quadratic equations. Ka = [HA] — х [НА] Classify these situations by whether the assumption is valid or the quadratic formula is required. Assumption is valid Quadratic formula is required Answer Bank [HA] = 0.001 M [HA] = 0.01 M Ka = 1 x 10¬4 [HA] = 0.1 M [HA] = 1 M [HA] = 0.01 M Ka = 1 × 10–5 Ką = 1 × 10-3 Ka = 1 × 10–3 Ka = 1 × 10-5
A Determine the [H+], pH, and pOH of a solution with an [OH-] of 0.00011 M at 25 °C. [H*] = pH = pOH = Determine the [H+], [OH-], and pOH of a solution with a pH of 3.79 at 25 °C. [H+] = [OH-] = pOH = Determine the [H]. [OH-], and pH of a solution with a pOH of 4.43 at 25 °C. [H+] = [OH-] = pH = M M M M M
Los Angeles has water regulations that requires any wastewater poured down the drain to be between pH = 4.5 and pH = 9.0. In lab, Dr. Smith is feeling lazy and decides to pour waste down the drain instead of going through the appropriate procedure for disposal of chemical waste. The waste contained your 0.250 M solution of HCl. Does this wastewater comply with the Los Angeles water standards? Hint: Recall that strong acids completely dissociate. HCl → H+ + Cl- How is [H+] related to the concentration of the HCl solution? a)No, this solution has pH below the safe range. b)Yes, this solution has pH within the safe range. c)No, this solution has pH above the safe range. d)The pH will depend on the volume (liters) of solution.
Calculate the pH of each of the following strong acid solutions. (a) 0.00532 M HCI pH: = (b) 0.794 g of HCIO4 in 33.0 L of solution pH = (c) 48.0 mL of 3.20 M HCl diluted to 3.20 L pH: = (d) a mixture formed by adding 54.0 mL of 0.00540 M HCI to 90.0 mL of 0.00120 M HCIO4 pH = =
4) please see attached
Can you please answer question 1
I need part D, E and F only
In aqueous solution the [H'] is 1.4 x 104 M. The [OH] in the same solution is A) 1.4 x 10-² M B) 1.4 x 10-7 M C) 1.0 × 10-7 M D) 7.1 x 10-1l M In aqueous solution the [OH-] is 3.0 x 106 M. The [H*] in the same solution is A) 1.0 x 10-" M B) 3.3 x 10-° M C) 3.0 x 10-6 M D) 3.0 x 10% M If an aluminum nitrate solution is added to a sodium fluoride solution the following equilibrium will be reached: Al³*(aq) + 6 F-(aq)=AIF6 (aq). For this equilibrium, K = 5.0 x 1023. Choose the correct equilibrium constant and the correct direction favored at equilibrium. A) K = [AIF,"] [A1³* ][F] ' 3+ ; reverse B) [AIF] K = forward [A1* ]F ]' [AIF,] [A1** ][FT C) K = reverse IDENAL D) [AIF,] K = [AI** ][F** ; forward
Calculate [OH -] and pH for each of the following solutions.(a) 0.0068 M NaOH [OH-] = M pH = (b) 0.0218 g of NaOH in 460.0 mL of solution [OH -] = M pH = (c) 83.6 mL of 0.00124 M Sr(OH)2 diluted to 400 mL [OH -] = M pH = (d) A solution formed by mixing 16.0 mL of 0.000250 M Sr(OH)2 with 89.0 mL of 7.6 x 10-3 M NaOH [OH -] = M pH =
Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for for pH to 2 decimal places. solution A B C [H₂O*] 8 1.5 X 10 mol/L mol/L 0.13 mol/L pH 8.27 x10 x Ś [H₂O+] to to 2 significant digits, and your entries
Hydrochloric acid is one of the common acids used in the laboratory. It is very strong acid and react with many substances including metals. a) Why is hydrocloric acid classified as a strong acid? b) Write a chemical equation to represent it action on zinc. c) What is observed when i. Litmus paper is dipped in hydrochoric acid ii. two drops of methyl orange is put in 20cm3 of 0.1M hydrochloric acid? iii. Hydrochloric acid react with calcium carbonate
Aq of NH4+ Aq of HF NH4+=6.25M HF=1.04x10^-6M NH3=5.00x10^-4M F=2.50x10^-5M H3O+=5.00x10^-4M H3O+=2.5x10^-5M What is the pH of both solutions? What is the concentration of OH- ions and the pOH of both solutions?