A solution with an OH| concentration of 1.20×10-7M has a pH of O 7.06 O 7.07 O 7.08 7.09

Q: Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?

A: Given, pH = 10.7 We know that, pH + pOH = 14                        => pOH = 14 - pH…

Q: The pH of lemon juice is about 2.0, whereas tomato juice's pH is about 4.0. Approximately how much…

A: Given values  pH of lemon juice = 2 pH of tomato juice = 4

Q: The pH of a 0.050 M aqueous solution of sodium benzoate falls within what range? Periodic Table and…

A: We have to calculate the range of pH of aqueous solution of sodium benzoate. 0.05 M aqueous solution…

Q: e pH of a solution  with [H+]  = 1.5x 10-1

A: The pH of the solution is a measure that how much the given solution is acidic and basic in nature.…

Q: a solution has a concentration of OH- =4.0x10-5 M. what are the concentration of H3O+ and the pH of…

A: pH of a solution can be defined as negative of logarithm of concentration of hydronium ions

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: (3 points) The pH of a sample of soap solution is 10.80. Calculate its molar hydronium…

A: 4th option is correct. Solution is given in step no 2:

Q: WHAT IS THE OH- CONCENTRATION OF A SOLUTION WITH A pH of 1.3? scientific notation.…

A: The concentration of a solution can be defined in terms of molarity as the ratio of the amount of…

Q: Calculate the pH of 1.0M NaHSO2 solution. (Ka1=1.2x10-2 ; Ka2=6.6x10-8). Show the complete solution

A: Given: 1.0M NaHSO2 solution (Ka1=1.2x10-2 ; Ka2=6.6x10-8) To find: pH of the solution.

Q: Which solution has the highest pH? O 0.065 M HIO (Ka-2.3x10-11) O 3.5x10-4M HBrO (Ka-2.5x10-9) O…

A:

Q: What is the H3O + concentration of an aqueous solution with a pH of 12.17 A. 6.8x10-13 B1.9x10-9…

A: Answer :  We have to calculate Concentration of H3O+ and pH of solution is given I.e 12.17

Q: 6. OH- concentration is 1.233x10(-7). What is the pH? 8.09 5.09 6.09 7.09

A: PH = -log [H+] POH= - log [OH-] Given [oH-]= 1.233×10-7

Q: Oven cleaner has a pH between 13 and 14. What two whole-number values of x should be used in…

A: pH = -log[H+]  so, [H+] = 10-pH

Q: The Kw for water at 0 °C is 0.12 × 10-14 M². Calculate the pH of a neutral aqueous solution at 0 °C.…

A: In this question, we have to calculate the pH of a Neutral solution at 0°C when Kw for water at 0°C…

Q: Calculate the pH of a solution that has [OH]= 1.0 x 10-8 M. Multiple Choice pH = 1.00 O pH = 7.00…

A: Introduction: The hydrogen ion concentration of a solution is expressed in terms of pH is calculated…

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 solution has [H​3O​+​​] = 4.5 x 10^-3M. Estimate the pH

A: pH = - log [H​3O​+​​]        = -log[ 4.5 x 10^-3]           = 3 - log 4.5             = 3- 0.653…

Q: A concentrated acid is fully neutralized with a dilute base. What is the most logical expectation…

A: Given that, a concentrated acid is fully neutralized with a dilute base. Now, when a solution is…

Q: Calculate the pH of a solution with a H3O+ concentration of 4.76 × 10-4 M.   3.32 10.68 5.45 4.76

A: Given, [H3O+] = 4.76 x 10-4 M

Q: What is the hydrogen ion concentration of a solution with pH 9.75? -10 [H*] = 8.37 x10

A: Given pH = 9.75

Q: 2. Complete the following table with the needed [H3O*], [OH]], and pH, and classify the solution as…

A:

Q: What is the pH of a solution with a concentration of 2.20 × 10-5 M H+? Report your answer to two…

A: Given, The concentration of H+ = 2.20 x 10-5 M. pH is the negative logarithm of hydrogen ion…

Q: Which aqueous solution has the lowest pH at 25 °C? 0.45 M H2S O 0.35 M HF O 0.34 M HOCIO O 0.33 M…

A: Answer :-  0.33 M HBr has lowest PH at 25 °C

Q: Indicate whether solutions with each of the following ionconcentrations are neutral, acidic, or…

A: Since the pH of solution is given by  pH = -log[H+] = 14 + log[OH-] And the solutions will be acidic…

Q: 06509 culate is the pH of a solution that has [H3O*] =4.16 x 10-3 M. 16 38 1.62

A:

Q: What is the pH of a solution that contains 2.54 x 10–4 M OH–? 11.46 6.40 2.54 3.60 10.40

A: We have to calculate the pH of Solution.

Q: Morphine is a weak base. A 0.150M solution of morphine has a pH of 10.7. What is Kb for morphine?

A: Morphine Molecular formula C17H19NO3 Morphine is a monobasic so it dissociates in aqueous solution…

Q: A strong acid solution is diluted by a factor of 100. Which statement below is true? The pH…

A: Answer

Q: Calculate the pH of each solution: (a) 0.0155 M HBr (b) 1.28 × 10-³ M KOH (c) 1.89 × 10-3M HNO3 (d)…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions  are…

Q: What is the pH of a solution that contains 3.78 x 10–4 M OH–? 10.22 6.58 10.58 3.78 3.42

A:

Q: 3. The [OH] of a solution is 5x10(-6) M. What is the pH? O 6.7 8.3 8.7 6.3

A: First of all, we will calculate the concentration of [H+] from ionic product of water and from there…

Q: What is the pH of a solution when the [OH^-] = 1 x 10^-3

A:

Q: [H30*] (M) [ОН] (М) pOH pH Acidic or Basic а. 0.0059 b. 12.00

A:

Q: The concentration of H3O+ in a solution is measured to be 6.27 x 10-3 Report the pH of the solution…

A: The pH of a solution is calculated by using the following expression: pH = -log[H3O+] where [H3O+]…

Q: Calculate the [OH-] in a solution with a pH of 6.59? * O 7.4 M O 6.6 M O 3.9 x 10^-8 M O 3.9 x 10^6…

A: pH in the calculation of H+ concentration. But we can evaluate HO- concentration also.

Q: the PH of a solution of HCl that is 1.0x10^-9 M at 25c is  a) 9.00 b) less than 7 c) 7.00 d) less…

A: The concentration of HCl acid is very very less i.e 1.0 X 10-9  So we can not directly say that the…

Q: What is the OH- ion concentration in a solution with pH = 4.75? O 6.78×10-8 M 5.62×10-10 M O…

A:

Q: A solution whose pH is equal to 4.0 has a hydrogen ion concentration of _____.  (A)1 x 104 M (B)1 x…

A: The pH of a substance is given by, pH = -log[H+]

Q: 19.For NaNO3, an aqueous solution will have a pH 1. greater than 7. 2. less than 7. 3. equal to 7.

A:

Q: Indicate whether the following solutions are acidic, basic, or neutral. 5x10 6 м нзо" 5х 10° м он 1х…

A: pH < 7 : Acidic solution  pH = 0 : Neutral Solution pH > 7 : Basic Solution      pH = - log…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 1.10 × 10-º M. pH

A:

Q: Determine the pH of a solution with an [OH-] = 3.6 x 10-10 M.

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

Q: A strong acid solution is diluted by a factor of 1000. Which statement below is true? The pH…

A: The strong acid solution contains hydrogen ions. One can define pH as, pH=-logH+ Let solution…

Q: A solution with (OH- )of 5 x 10^3 has a pH of? A.-2.3.   B. 11.7.   C 7.0. D. 2.3

A: (b) 11.7 Concentration of OH- ions = 5×10-3 Now, pOH = -log[OH-]                    = -log (5×10-3)…

Q: 3) Calculate the [OH-] in a solution with a pH of 6.59? a) 7.4 M b) 6.6 M c) 3.9 x 10^-8 M d)…

A: Given      PH  = 6.59  [ OH- ]  =  ?

Q: 1) The pH of rainwater is 5.82. The [H*] is A. 6.61x10-09 C. 1.51x10-06 B. 6.16 x10-09 D. 1.15…

A:

Q: Calculate the pH of a 0.400M solution of quinoline, C₉H₇N.

A:

Q: Calculate the concentration of all species (other than water) present in a 0.500 M phosphoric acid…

A: Phosphoric acid is a tribasic acid.It undergoes dissociation in three steps, resulting in various…

Q: alculate the [H3O+] and [OH-] for a solution with each of the following pH values: a. 3.00 b. 6.2 c.…

A: PH = - log [H3O+] Then [H3O+] = 10-PH  OH-= 10-14H+ NOTE- As per our company guideline we can answer…

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.