In an aqueous solution at 25°C, if [H₃O⁺] = 6.2 × 10⁻⁴ M, then [OH⁻] is:

Q: What is the pH of a 0.310 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: Recall the expression of pH for weak acid as follows   pH=12pKa-12logC Here HF is a weak acid with…

Q: What is the pH when the [OH-] = 4.26 x 10-2 M at 25 oC?

A: 1- First we need to calculate the pOH of the solution :  We know that,  pOH = -log[OH-]  pOH = -log(…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 5.3 × 10⁻⁴ M, then [OH⁻] is:

A: Given [H3O+] = 5.3*10^-4 M  Kw = [ H3O+][OH-]

Q: What is the pH of a solution that has [H3O+]=1.0 x 10^-11?

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.4 × 10⁻⁴ M, then [OH⁻] is:

A: The concentration of OH- can be calculated as:

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]=3.3*10^-3 M

A: pH of the solution is given by,                               By using given concentration to get…

Q: Calculate [ OH− ] for a solution where [H3O+]=0.00605 M .

A:

Q: Determine the [OH−], pH, and pOH of a solution with a [H+] of 7.3×10−8 M at 25 °C.

A: Given :- [H+] =7.3×10^−8 M  To calculate :-  [OH−], pH, and pOH

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 2.3 × 10⁻⁴ M, then [OH⁻] is:

A: Here given---- [H3O+] = 2.3 ×10-4 M [OH-] = ? We know, dissociation of water occurs as---- H2O…

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that -  Hydrogen ion concentration , [H+] are -  a) 0.01 b)1.0 x 10 –8  c) 4.67 x 10 –4  Then,…

Q: What is the pH of an aqueous solution if the [H+] = 0.1M?

A: Given Data :  [H+] = 0.1M  To calculate : pH.  Formula : - log [H+]

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 is the pH of a 0.330 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: The objective of this question is to calculate the pH of a 0.330 M solution of HF. The Ka value for…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 7.6 × 10⁻⁴ M, then [OH⁻] is:

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Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

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Q: What is the pH of a 0.480 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.2 × 10⁻⁴ M, then [OH⁻] is:

A:

Q: Calculate either [H3O+] or [OH¯] for each of the solutions at 25 °C. Solution A: [OH-] = 1.57 × 10−7…

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Q: Determine [OH-] in a solution where [HNO3] = 0.892 M.

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.3 × 10⁻⁴ M, then [OH⁻] is:

A: [OH-] = 7.7 x 10-11 M

Q: Calculate the  [ H3O+ ]  of an aqueous solution that is  3.0  ×  10−9  M in OH−.

A:

Q: What is the pH of a 0.440 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: In an aqueous solution of HF, the dissociation of weak acid HF and autoionization of water takes…

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.3 × 10⁻⁴ M, then [OH⁻] is:

A: Using ionic product of water, concentration of hydroxyl ion can be determined from the hydronium ion…

Q: Calculate the hydroxide ion concentration ormic acid. (Assume that K¿ (HCOOH) OH-1 of an aqueous…

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Q: In an aqueous solution at 25 C, if [H3O+]=3.1×10^-4M, then [OH-] is

A: Given data: The hydronium ion concentration is H3O+=3.1×10-4 M. To find: The hydroxide ion…

Q: Determine [OH-] in a solution where [Ba(OH)2] = 0.0249 M.

A: Strong Base - A base which completely dissociates into it's ions in aqueous solution called strong…

Q: The OH- concentration in an aqueous solution at 25 celcius  is 7.1 x 10^-5. what is [H+]?

A: Given,  Concentration of OH-ion = [OH-] = 7.1 x 10-5 M  What is [H+] = ?

Q: Determine the [OH¯], pH, and pOH of a solution with a [H*] of 2.1 × 10-¹² M at 25 °C. [OH-] = pH =…

A: given H+ = 2.1 x 10-12

Q: At 25°C, what is the hydroxide ion concentration, [OH−], in an aqueous solution with a hydrogen ion…

A: Given,The hydrogen concentration, [H+] = 3.1 x 10-9 M

Q: Betermine the [HT] = [OH-] = pH = 2 and pH of a solution with a pOH of 4.98 at 25

A: We can determine the [H+] , [OH-] and pH from pOH using the following formulas : pH +pOH = 14 pH =…

Q: An aqueous solution of a strong base has pOH 1.76 at 25°C. Calculate the concentration of base in…

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Q: What is the pH when the [OH-] = 7.33 x 10-9 M at 25 oC?

A: POH = -log[OH-]  PH + POH = 14

Q: 54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify…

A: Since, you have given multiple subparts, we will solve the first 3 subparts for you. For other parts…

Q: Calculate the [OH-] of [H+] = 5.4 x 10^-5 M at 25 degrees Celsius. Identify the solution as neutral,…

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Q: Determine [OH−] , pH , and pOH of a 0.21 M ammonia solution. For NH3 , Kb=1.76×10−5.

A: [OH-] = 0.001922 M  pOH = 2.72  pH  = 11.28Explanation:

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 8.2 * 10^-4 M

A: pH of the solution is given by,                     By using given concentration to get the pH of…

Q: Determine [OH−], pH, and pOH of a 0.25 MM ammonia solution. For NH3, Kb=1.76×10−5.

A: The question is based on the concept of equilibrium. ammonia is a weak base. so, partially…

Q: Calculate the pH of a 7.1 x 104 M solution of HC104, a strong acid, at 25°C. pH =

A:

Q: Determine [OH-] in a solution where [HNO3] = 0.472 M.

A: Given: [HNO3] = 0.472 M We have to determine the [OH-] in the solution.

Q: Calculate the percent ionization of a 0.437 M solution of hypochlorous acid. (Assume that Ka (HClO)…

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Q: Calculate the percent ionization of a 0.524 M solution of hypochlorous acid. (Assume that K sub a…

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Q: The molar concentration of OH- in a water solution is 1.5 × 10−9 M. Determine the concentration of…

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Q: Calculate the following for the given aqueous solutions at 25.0 oC:​a) The [H+] concentration of an…

A: Given a)  pH = 1.02 ( as pH cannot be negative ) b) Concentration of HNO3 = 7.27 × 10-8 M

Q: Determine [OH-] in a solution where [Ba(OH)2] = 0.0359 M.

A: Strong electrolytes are the electrolyte which completely dissociates into ions.

Q: What is the pH when the [OH-] = 7.33 x 10-9 M at 25 oC?

A: The formula for the pOH calculation is : => pOH = -log[OH-]