A solution has [H+] = 3.5x10-4 M. The [OH-] in the solution is what?

Q: What is the pH for a solution at 25°C that has [OH-]=8.23×10-5-M

A: pH is a measure to calculate the extent of acidity of a solution. It is the negative logarithm of…

Q: A solution has a [H3O+] of 0.0015 M. Calculate the [OH-], the pH, and the pOH of the solution. Is…

A: In the question is given that concentration of [H3O]+  is 0.0015. i.e. [H]+ = 0.0015 [OH]- = ? pH =…

Q: What is the [OH-] if the [H+] concentration is 3.1x10^-4 Molar?

A: The concentration of H+ ions is 3.1×10-4 M. The relationship between the concentration of H+ ions…

Q: what are [H+] and [OH-] in a 2.86 M solution of HBr

A: [H+].[OH-] = Kw  [H+].[OH-] = 1 × 10-14

Q: The pOH of a basic solution is 3.03 what is the [OH-]?

A: Given :- pOH of basic solution = 3.03  To calculate :- concentration of OH- ions i.e. [OH-]

Q: Find the [OH-] in an acidic solution where [H+] = (6.0x10^-5)

A: An acid is a molecules which can donates protons or they are capable of donating hydrogens. Bases…

Q: calculate the [H3O+] value {OH-]=1.2x10-5M

A: [OH-] = 1.2 × 10-5 M  [H3O+] = ?

Q: Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.49 × 10−7…

A:

Q: What is the pH of 2.2 x 10-3 M HC1?

A:

Q: A solution has [OH-] = 1×10-5. What is the concentration of H3O+ ion?

A:

Q: 4) What is the [OH] for a solution with a [H,O'] of 9.97 X 104 M? Is the solution acidic, basic or…

A:

Q: Calculate [OH¯] for a solution where [H,O*] = 0.00409 M.

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

Q: What is the [ H3O+] in a solution that has a [OH-] = 9.0×10−2 M?

A: Given, Concentration of OH- = 9.0 * 10-2 Concentration of H3O+ =? By using the autoionization…

Q: What

A:

Q: If [H+] = 2.9 x 10-5 M in a solution, what is the [OH-]? 2.9 x 10^-5 M 4.7 x 10^-8 M 2.9 x 10^9 M…

A: Given, [H+] = 2.9 x 10-5 M We know, => pH = -log[H+] on substituting the value=> pH = -log(2.9…

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A:

Q: What are [H+] and [OH-] in a 0.00338 M solution of KOH

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What are the hydronium and hydroxide ion concentrations in a solution whose pH is 7.95? [H*]. [OH-]-

A:

Q: Determine [OH−][OH−] of a solution that is 0.220  in HCO3−HCO3−. (Ka1 for H2CO3H2CO3 is…

A: Given,molarity of HCO3- = 0.220 MKa1 of H2CO3 = 4.3 x 10-7H2CO3 (aq) + H2O (l)    HCO3- (aq) + H3O+…

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: What is the [OH-] in a solution that has a [ H3O+] = 2.0 × 10-4 M? Is this solution acidic, basic,…

A:

Q: At 25 degrees C, a solution has a pH of 10.69. What is the [OH-] in the solution?

A: Given : pH = 10.69

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the [H3O+].

A: Given: The concentration of hydroxide ions is provided,i.e. [OH-] = 1.0 x 10-5 M. The hydronium ion…

Q: A solution has [H⁺] = 4.9 10⁻³ M. The [OH⁻] in this solution is A) 1.0 10⁻¹⁴ M B) 4.9 10⁻¹¹ M C) 4.9…

A: Given is, [H⁺] = 4.9 ×10⁻³ M

Q: Calculate the [OH-] of a strong acid solution that is 8.8 x 10-3 M HCl.

A:

Q: In a(n) neutral solution, the concentration of H3O+ is _____ the concentration of OH-. -greater…

A: Given statement : in a(n) neutral solution, the concentration of H3O+ is _____ the concentration of…

Q: Calculate [H3O+] when given the [OH-] in each of the following aqueous solutions and classify the…

A:

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A: The auto ionization constant of water is shown below: OH- H3O+ = KwOH- H3O+=1×10-14

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A: The pH of solution indicates the acidity or basicity of the given solution, which is the negative…

Q: Determine the [OH-] in a solution with a pH of 4.358.  Your answer should contain 3 significant…

A: The relationship between the pH and [OH-] is given by  pH = 14 + log[OH-]  where [OH-] =…

Q: What are the [H+] and [OH-] concentrations in a 125 mL solution prepared with 0.100 mol of HI and…

A: The molarity of the solution is defined by the mole of solute present in one liter of solution. The…

Q: A solution has a [H 3O +] of 1.024x 10 -10 M. What is the [OH -]?

A: PH= - log [H 3O +]  POH=log [OH -]

Q: Calculate [OH−] for the strong base solution formed by mixing 13.0 mL of 1.00×10−2 M Ba(OH)2with…

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Q: What are [H*], [OH-] and pH in a solution with a pOH of 12.11 15.

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Q: Calculate the [OH-] in a NaOH solution with a pH of 12.73                           Group of…

A: POH is equal to negative logarithmic value of hydroxide ions concentration

Q: What is the relationship between H+ and OH- concentrations in a solution that has a pH of 11?

A:

Q: Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the [H3O+].

A:

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: What is [OH ] in a 0.0058M HI solution?

A: The dissociation of HI takes place as,                                             HI (aq) ---->…

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.