Determine the [OH-] of a solution when the [H+] = 4.0 x 10-8

Q: the concentration of OH-is one-hundredth what it was at pH 5. the concentration of H+ is twice what…

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Q: Methylamine is a weak base that ionizes according to the equation CH3NH2 (aq) + H2O(l) ⇄ CH3NH4+…

A: Given, 0.1 M solution of CH3NH2

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: Rank the solutions in order of decreasing [H3O+]: 0.10 M HCl;0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.

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Q: 6. Calculate the pH from the (OH-1 for each of the following [OH-1 7.2x103 pH (OH-1 pH 3.5 x 104 3.6…

A: PH is defined as negative logarithm of concentration of H+ ions.

Q: Which of the following (assuming the same concentration in water) would make a solution with the…

A: Strong acid: Strong acids completely dissociate into their ions in water. Let HA is strong acid then…

Q: If [H+] = 9.1x10^-4 M, what is [OH-]?

A: Given that, [H+] = 9.1x10^-4 M We have the following relationship between [H+] and [OH-]

Q: When would a solution be basic? [H+] > [OH-] When the pH is from 7 to 14 [H+] = 1 × 10-7

A: A solution is basic, when an aqueous solution contains more hydroxide (OH-) ions than that of H+…

Q: What is the [ H3O+] in a solution with [OH-] = 1 × 10-12 M? Group of answer choices 1 × 102 M…

A: We know that the relationship between [ H3O+]& [OH-]. kw= [H3O+] [OH-] = 1x10-14  [H3O+]…

Q: If the pH of a solution is 10.820, what is the [OH-] in the solution a. 1.5x10-11 M b. 1.51x10-11 M…

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Q: Rank the following solutions according to their acidity:   Rank Solution 1 [H3O+] =10^-8 M…

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Q: Write equations showing how each of the following weak bases ionizes water to form OH− 1. NH3 2.…

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Q: 1. If [OH-]= 6.8x10^-11M Find [H3O+], pH 2. If pH= 8.9 Find [H3O+], [OH-]

A: Using formula of pH And using realtion between [H3O+] and [OH-] we can solve this problem.

Q: What is the [OH-] of a solution with pH = 3.17? a. 1.48 x 10-10 M b. 6.76 x 10-4 M c. 1.48 x 10-11…

A: To calculate the hydroxide ion concentration first of all we calculate the pOH of the solution and…

Q: If the [H3O+] concentration is 8.3x10-9, what is the [OH-] concentration?

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Q: An aqueous solution at 25 °C has a H,0" concentration of 4.2 × 10 M. Calculate the OH concentration.…

A: Solution : We should know that  [H3O+][OH-]=Kw=1×10-14 Given, [H3O+]=4.2×10-6

Q: 2. What is the pOH of a solution in which the hydroxide ion concentration is 3.2x10-3M? 3. What is…

A: POH = -log[OH-] [H]+[OH-] = 10-14 M2

Q: If the [ H+  ] concentration of a water sample is 1 x 10-4 M, the [ OH- ] concentration is:________

A: GIven: The concentration of hydrogen ion [H+]=1 x 10-4 M The concentration of hydroxide ion i.e.  […

Q: What is the OH- concentration of a solution  with a H3O+ concentration of 8.47x 10-8

A: Given concentration of H3O+ is 8.47 × 10-8  [H3O+] = 8.47 × 10-8

Q: What is the hydroxide (OH-) concentration of a solution with a hydronium (H3O+) concentration of 4.7…

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Q: Tell the concentration and if it’s an acid or base 1. [OH-]=5.48 X 10 ^-9 M 2.[OH-]=2.0 X 10^-13 M

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Q: Convert 5.80  pH value to OH- concentration (in μM).

A: Answer :-  Concentration of OH- ion = 6.31 × 10-3 (μM)…

Q: Which of the following states the correct [H+] and [OH-] at pH 10.0? a) [H+] = 4 M;  [OH-] = 10 M…

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Q: Rank the following solutions according to their acidity:   Rank Solution 1 pH=9     Solution 2…

A: Rank the following solutions according to their acidity:

Q: A water sample collected from the UST Fountain of Wisdom has an OH- concentration of 3.1 x 10-8 M.…

A: pOH is defined as the negative logarithm of hydroxide ion concentration present in the solution.…

Q: A solution has (OH)-1-10 What is the concentration of H0 ion? mol/L

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Q: Given each [OH-] below, what is the [H3O+]: 0.0359 1.41x10-3 3.89x10-6 4.255x10-6 8.65x10-5…

A: Given information, 0.0359 1.41x10-3 3.89x10-6 4.255x10-6 8.65x10-5 1.86x10-13 2.193x10-3

Q: Of the following solutions, which are acidic? 1) pH = 2 2) pH = 7 3)[OH-] = 10-7 M 4) [H3O+] =…

A: At 25˚C The solutions having pH <7 are acidic. The solutions having pH >7 are basic. At pH =…

Q: What are the [H3O+] and [OH-] concentrations respectively in a 0.200 M aqueous Hal solution? Kw=…

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Q: What is the (OH-) of 0.1M HCl solution?

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Q: A solution has a hydronium concentration of 7.50 x 10-5. What is the hydroxide concentration in M?

A: Given = Hydronium ion concentration (H30 +) =7.50*10-5 Hydroxide ion concentration (OH-) =?

Q: An aqueous solution at  25°C  has a  H3O+  concentration of  ×1.110−7M . Calculate the  OH−…

A: The pure water equilibrium can be written as follows: 2H2O(l)⇌H3O+(aq)+OH−(aq) The value of the…

Q: Calculate the [H+1]for this solution.

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Q: Calculate [OH-] given [H3O+]. [H3O+] = 1.5 x 10-9 M       [H3O+] = 9.1 x 10-4 M

A: Given, the concentration of hydronium ions as follows,a) [H3O+] = 1.5 x 10-9 M        b) [H3O+] =…

Q: Calculate the pH of a solution in which [ OH^- ] = 2.50 x 10^-14

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

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Q: Convert each of the following OH- concentrations to pH. 1.1M 2.5 uM 0.030M

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question…

Q: calculate the [OH-] of a solution that has [OH+] = 6.2 × 10-6 M at 25°C PLEASE ANSWER EVERYTHING ON…

A: Note: as per guidelines if multiparts question, first three only allowed, please post questions…

Q: Dimethylamine (CH3-NH-CH3) is a weak base with a Kb = 5.9 x 10-4.  Determine the concentration of…

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Q: Concentration What You Have [H*] [OH-] pH pOH 0.1 M H+ 01M 0.32 M OH- 0.32 M 6.5 x 10-2 H3O+ 4.6 x…

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Q: Which of the following solutions is most basic? Group of answer choices [OH-] = 1 X 10-4 [H+] = 1…

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Q: Calculate the pH of a 0.53 M HONH2 solution. Give your answer to two decimal places Kb(HONH2) = 1.0…

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Q: [OH] - 1.6 x 10 8 M [H*]- M PH - POH - [OH']-8.2 x 10 12 M [H*)- DH - POH -

A: Interpretation- To determine the  concentration of [ H+ ] , pH and pOH in the given question.…

Q: Calculate the [OH-] and the pH of a solution with an [H*] = 8.2 × 10-12 M at 25 °C. -9 [OH"] 1.2 x10…

A: Answer given as follows

Q: Tell whether each of the following statements is characteristic of an acid or a base. 1. Neutralizes…

A: According to Arrhenius theory - Acids produce H+ ions in their aqueous solutions. Bases produce OH-…

Q: The [H3O+] is 6.2x10-5 M; so the [OH-] is 1.6x10-10. True or false

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Q: Determine the [OH^-] of a solution when the [H+] = 4.0 x 10^-8

A: The concentration of  [H+] = 4.0 x 10–8

Q: Calculate the hydronium concentration from the following hydroxide concentration [OH^-] = 4.53 x…

A: Given, Hydroxide concentration, [OH-] = 4.53 x 10-9 M Hydronium concentration [H3O+] = ? Formula…

Q: Given [OH-] = 1.75 x 10-4M, calculate [H3O+]. A. 1.25 x 10-4M B. 8.0 x 10-11M C. 5.71 x 10-11M…

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Q: pOH of a 10-1 M HCI solution is: O -13 O -1 O 13 O 1

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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.