Answered: Rank the following solutions from the…

Rank the following solutions from the lowest pH to the highest pH А. 1.2х105 М NaOH 9.07 В. О.0015 М HCI С. 0.13 М НF D. 7.1x107 M Sr(ОНH)2

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 68AP: Which of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH]...

See similar textbooks

Related questions

Q: A chemist makes four successive 1:10 dilutions of 1.0X10⁻⁵ M HCl. Calculate the pH of the original…

A: The pH of a solution is the negative of logarithm of the concentration of hydrogen ions in the…

Q: A certain weak base has a K, of 7.20 x 10-7, What concentration of this base will produce a pH of…

A: Base dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

Q: A chemist dissolves 715. mg of pure potassium hydroxide in enough water to make up 80. mL of…

Q: pH = –0.36 [H+] = ____ M [OH - ] = _____ M b pH = 9.40 [H + ] = _____ M [OH - ] =…

Q: For solutions with the following pH values, determine the [OH-] for the solution. (Hint: This will…

A: We have to calculate the concentration of the OH- ion, [OH-] in the given solution. The pH of the…

Q: A chemist dissolves 843. mg of pure potassium hydroxide in enough water to make up 80. mL of…

A: Mass of KOH = 843 mg1mg = 10-3 gMass of KOH = m = 0.843 gMolar mass of KOH = 56.1 g/mol = MMoles of…

Q: ndicate whether the solutions listed below are acidic, basic, or neutral. pH = 2.13…

A: For acidic species, pH < 7,For neutral species, pH = 7, and for basic species, pH > 7.

Q: Calculate the pH of a formic acid solution that contains 1.35% formic acid by mass. (Assume a…

Q: A solution of formic acid (HCOOH, K, = 1.8 ×10*) has a pH of 2.70. Calculate the initial…

A: Given, Ka = 1.8 x 10-5 pH = 2.70 We know that, pH can be expressed as negative…

Q: A chemist dissolves 858. mg of pure sodium hydroxide in enough water to make up 170. mL of solution.…

A: The pH of any solution is defined as the negative logarithm of the H+ ion cocentration of the…

Q: Which of the following statements is false regarding a solution of 1.0 M HNO3? [H+]=1.0M pH=0…

A: 1.0 M HNO3 HNO3 (aq)------> H+ (aq)+ NO3- (aq) pH = - log [H+] Here , [H+] = 1.0 M

Q: Which pH or pOH value is INCORRECTLY matched with its description? O pH = 1.32 / distinctly acidic O…

A: We know that ; pH < 7 : Acidic pH = 7 : Neutral pH > 7 : Basic By this we identify that , the…

Q: Sapling Learning | Lenoir-Rhyne | X y! Yahoo - login acid or base calcul 17.3: Acid-Base Tit y!…

A: 1) Since moles = molarity X volume in L Hence moles of HCl mixed = 0.35 X 35 / 1000 = 0.01225 And…

Q: Calculate the H,O* concentration for each pH. pH = 11 [H,O*] = M pH = 1 [H,O*] = M M pH = 7 [H,O*] =

A: a) pH = 11 b) pH = 1 c) pH = 7 We know that, pH of solution is :- pH = -log[H+] pH = -log[H3O+]

Q: A 0.145 M solution of a weak base has a pH of Part A 11.27. Determine Kb for the base. Express your…

A: Given that : Molarity of weak base = 0.145 pH = 11.27 We have to determine the Kb for the base.

Q: Given that Ka for HCN is 6.2×10−10, calculate Kb for CN-. Express your answer to two significant…

A: 1- First question, Calculate the value of Kb for weak base CN- ion : We know that, Kb × Ka = Kw Kb…

Q: Determine the pH of the HCI solution in the chemical cabinet that is 27% by mass. (Density of H,0 =…

A: The relation between percentage, density and molarity of any solution is : Molarity = (% x 10 x…

Q: A certain weak base has a K, of 8.90 × 10-7. What concentration of this base will produce a pH of…

A: Concentration of base required can be calculated using equation: [OH-] = √(Kb × [Base])

Q: Use this data to rank the following solutions in order of increasing pH. In other words, select a…

A: For salt of weak acid and strong base. pH = 7+{pKa + log[Salt]}/2 And pH>7 For…

Q: Calculate the pH of a solution that has [H301 = 3.1 × 10-8 M. A) pH 3.18 B) pH = 3.10 C) pH 7.51 pH…

A: Answer

Q: If the following are dissolved in water, classify the resulting solutions as acidic, basic, or…

Q: Determine the pH of each solution.a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M KOH d. 0.245 M…

A: Given:- To determine the pH of solution a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M…

Q: Determine the pH of the HCl solution in the chemical cabinet that is 27% by mass. (Density of H2O =…

A: The pH of a given solution is the hydrogen ion concentration in the acidic solution and OH- ion…

Q: (References) A typical vitamin C tablet (containing pure ascorbic acid, H2C6H606) weighs 500 mg. One…

A: The question is based on the concept of equilibrium. we have been given a weak acid ascorbic acid.…

Q: A chemist dissolves 818. mg of pure potassium hydroxide in enough water to make up 150. mL of…

Q: Determine the pH of the HCl solution in the chemical cabinet that is 27% by mass. (Density of H2O =…

A: Molar mass of HCl = 36g/mol Density = Mass/Volume Density = 1.150 Mass = 1.150 x V Mass in the…

Q: Acids & Bases: Understanding Connections Between Descriptions of Weak Acid Dissociations When a…

A: The acid can be represented as HA. Acid dissociation is given. Here, one mole of acid dissociate to…

Q: A chemist dissolves 423. mg of pure potassium hydroxide in enough water to make up 130. mL of…

A: Given data, Mass of pure potassium hydroxide (KOH) = 423 mg Volume of solution = 130 mL…

Q: Determine [OH], [H*], and the pH of each of the following solutions. а. 2.1 М CSCI (OH] = |M [H*] =…

Q: Sapling Learning | Lenoir-Rhyne | X y! Yahoo - login acid or base calcul 17.3: Acid-Base Tit y!…

A: A 0.760 g of diprotic acid is dissolved in water and titrated with 0.260 M NaOH. The molar mass of…

Q: A chemist dissolves 722. mg of pure potassium hydroxide in enough water to make up 140. mL of…

Q: Sapling Learning | Lenoir-Rhyne | X y! Yahoo - login acid or base calcul 17.3: Acid-Base Tit y!…

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: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

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

Q: For each of the following solutions A. identify as either acid or base; B. calculate the…

A: We know that if, pH < 7, solution is acid pH > 7, solution is base. So, pH = 6.290 is acid pH…

Q: Which solution is most acidic (that is, which one has the lowest pH)? 0.30 M HF 0.60 M HF 0.30 M HBr

Q: A chemist dissolves 715. mg of pure sodium hydroxide in enough water to make up 110. mL of solution.…

A: To calculate the pH of the given sodium hydroxide solution, first of all, we calculate the molar…

Q: A chemist dissolves 190. mg of pure nitric acid in enough water to make up 190. mL of solution.…

A: Given : mass of nitric acid i.e HNO3 = 190 mg = 0.190 g…

Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

A: Given that: molarity of formic acid = 0.1 M Volume of solution = 400 mL Ka = 1.74×10-4 M.wt of…

Q: Be sure to answer all parts. What H3O+ concentration corresponds to each pH value: a) PH:2…

A: Given: pH values 2, 7 and 3. To Find: Concentration of H3O+ Solution: As we know, there is a…

Q: A chemist dissolves 382. mg of pure sodium hydroxide in enough water to make up 70. mL of solution.…

A: Solution : We need to calculate the molarity of the solution first 1M NaOH=40g of NaOH in 1 L of…

Q: 15. List all the species present in a solution that is 0.25 M in NH,Br and 0.25 M in KBr. Rank the…

A: In this question , we have given a solution containing 0.25 M NH4Br and 0.25 M KBr. We have to…

Q: OM aqueous solutions of the following salts be acidic , basic or neutral? ea solution is neutral if…

A: As you not specified so I am giving answer of first three subparts A) H2S is weak acid and ammonia…

Q: ou are given the following ; KBr, NH3, NaOCl, NH4Cl they are all 1 M aqueous solutions some other…

A: The given four compounds are KBr, NH3, NaOCl, NH4Cl. The concentration of each compound in the…

Q: A certain weak base has a K, of 7.20 × 10-7. What concentration of this base will produce a pH of…

A: Given Kb = 7.20 x 10-7 pH = 10.14 we know pH + pOH = 14 pOH = 14 - 10.14 = 3.86 and [OH-] =…

Q: A solution is prepared by adding 51.0 mL concentrated hydrochloric acid and 19.9 mL concentrated…

A: Given, Solution is prepared by adding: 51mL of 38% by Mass HCl solution 19.9 mL of 70% by mass HNO3…

Q: A chemist dissolves 307. mg of pure perchloric acid in enough water to make up 200. mL of solution.…

A: Perchloric acid is HClO4 Given : Mass of HClO4 added = 307 mg = 0.307 g…

Q: certain weak base has a ?b of 7.80×10−7. What concentration of this base will produce a pH of…

Q: following solutions. 0.20 M KCHO2 (Ka(HCHO2)=1.8×10^−4) Express your answer

A: Ka = 1.8 ×10-4 pKa = -log(Ka) = -log(1.8×10-4) = 3.74 Concentration of Salt(C)= 0.20 KCHO2 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

Rank the following solutions from the lowest pH to the highest pH
А. 1.2х105 М NaOH 9.07
В. О.0015 М HCI
C. 0.13 M HF
D. 7.1x107 M Sr(OH)2

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 with 2 images

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

Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
A 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000
A 0.050-M solution of the salt NaB has a pH of 9.00. Calculate the pH of a 0.010-M solution of HB.
A solution of formic acid (HCOOH, Ka = 1.8 104) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH], and the pH for this solution. [Hint: Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/mL.
Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
Two strategies are followed when solving for the pH of an acid in water. What is the strategy for calculating the pH of a strong acid in water? What major assumptions are made when solving strong acid problems? The best way to recognize strong acids is to memorize them. List the six common strong acids (the two not listed in the text are HBr and HI). Most acids, by contrast, are weak acids. When solving for the pH of a weak acid in water, you must have the Ka value. List two places in this text that provide Ka values for weak acids. You can utilize these tables to help you recognize weak acids. What is the strategy for calculating the pH of a weak acid in water? What assumptions are generally made? What is the 5% rule? If the 5% rule fails, how do you calculate the pH of a weak acid in water?
Write the formula and name for the conjugate acid of the following substances. (The information in Tables 15.6 and 15.8 may be helpful.) (a) N2H4 (b) NO2 (c) ClO4 (d) I
. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions. a. 1.10 M NaOH b. 2.0104M KOH c. 6.2103M CsOH d. 0.0001 M NaOH