If a solution has pH of 5.50, calculate its [OH-]*

Q: Calculate the pH of a solution with [OH-]= 4.6x10-5 M

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: Determine the [H*], [OH¯], and pH of a solution with a pOH of 7.10 at 25 °C.

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Q: Calculate [H3O+] for each solution pH = 1.52?

A: pH = -log [H3O+]

Q: Write an equation showing the dissociation of HC2H2O2I and calculate the pH of a 0.425M solution.

A: HCH2O2I is named as 2-iodoethanoic acid , which is a weak acid.  So we would first write it…

Q: Calculate the [H3O+] and [OH−] of a sodium hydroxide solution with a pH = 12.00.

A: • The values provided in the question are:-      i) pH of a NaOH solution = 12.00    • We need to…

Q: if the pH is 1.87 find the pOH, [H3O+], and [OH-] calculation

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Q: the Ph of a 0.050 M weak acid solution is 5.25. Calculate the Ka of the acid.

A: Given, pH of weak acid= 5.25 [weak acid ] =0.050 M Ka = ?

Q: Calculate the pH of a solution that has a pOH of 8.70.

A: Given,  pOH of the solution = 8.70  Calculate the pH of the solution = ?  Use the formula :  pH +…

Q: Determine if this solution is acidic or basic and find the pH, [OH], and the [H] if the pOH = 9.38

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Q: Calculate the pH of a solution that is .0400M in  a.) H3PO3  b.) H2S

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Q: Calculate the concentration of all species in 0.025 M H,PO, [H,PO,). [H_PO, ], [HPO, ]. [PO,"].…

A: Given, Initial concentration of H3PO4 = 0.025 M

Q: A concentration of HNO3 0.107M. What is the pH of this solution?

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: Calculate the H+ ion concentration in a solution with a pH of 3.85.

A: Given values -> pH = 3.85

Q: If the pH of a solution is 8.85, what is the concentration of hydroxide ions in the solution?

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Q: Determine the [H3O+] for solutions having the following pH value.  pH = 9.345

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Q: Calculate the pH of solution where [H] = 0.000023

A: pH measure the acidity of the solution.

Q: What is the pH of a solution if the concentration of H+ is .000284

A: Given :  Concentration of H+ = 0.000284 Therefore [H+] = 0.000284

Q: Calculate the hydroxide ion concentration, [OH"], for a solution with a pH of 11.35.

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Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

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Q: The weak acid, H A, has aKa value of 3.80E-3. Calculate the pH of the solution if the concentration…

A: The pH of a solution gives the measure of its acidity. More is the pH, less is the acidic character…

Q: Calculate pH of [H+] concentrations of 5.42x10-6 M and 9.98x10-12 M.

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Q: Calculate the [OH in a solution that has a pH of 2.92.

A: We know that, pH can be expressed as negative logarithm of H+. i.e.,                      pH = -…

Q: What is the pH of the following solution. 0.035 M HNO3

A: Given data contains, Molarity of nitric acid is 0.035 M.

Q: What is the pH value of solution if 0.24g NaOH is dissolved in 400ml of solution

A: Given weight of NaOH = 0.24 g  Volume of the solution = 400 mL  In the calculation of pH we have to…

Q: Calculate the  [ H3O+ ]  and  [ OH− ]  of a sodium hydroxide solution with a pH = 12.00.

A: The pH is calculated using the expression: pH  = - log [H3O+] The hydronium ion concentration can be…

Q: Calculate the concentration of H+ in an aqueous solution with a pH of а. 3.40 b. 9.20

A: Recall the following expression of pH         pH=-logH+ Here, H+ is concentration of H+ ion in the…

Q: Calculate the concentration of an aqueous solution ofNaOH that has a pH of 11.50.

A: Given: pH of NaOH solution is 11.50

Q: c). B (if basic).o

A: Reaction of Salt in Water, K2C2O4(aq.) + H2O(l)--->  2KOH(aq.) + H2C2O4(aq.)

Q: Calculate the [H*] in a solution that has a pH of 9.16.

A: Given :- pH of solution = 9.16  To calculate :- [H+] i.e. hydrogen ion concentration

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH¯], of 7.73 × 10-5 M.

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

Q: Given the pH = 6.0, find the [H3O+] concentration.

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Q: Calculate the pH of 0.0250 M NaOH.

A: NaOH being a strong base easily dissociated into its respective ions in water. NaOH -------> Na+…

Q: If a certain solution has a pH of 3.35, what would be its hydrogen ion concentration?

A: Given :- pH of the solution = 3.35  To be calculated :- Hydrogen ion concentration i.e. [H+]

Q: Calculate [H3O+] for a solution with a pH of 8.37.

A: The given data contains, pH =8.37

Q: An aqueous solution has a pH of 3.75. What is the hydronium ion concentration of the solution? Is it…

A: The question is based on the concept of PH and pOH calculations.   pH is defined as negative…

Q: A solution with a pH of 2.17 is

A: Given :- pH of solution = 2.17  To identify :- Nature of solution i.e. acidic, basic or neutral

Q: 2. Calculate the pH of the solution given that the molar hydroxide ion concentration is [OH]= %3D…

A: Given :- [OH-] = 0.000031 M  To calculate :- pH of solution  pH + pOH = 14

Q: What is the pOH of a solution that has a pH of 9.35?

A: •The values provided in the question:-      i) pH of a solution = 9.35      • We need to calculate…

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

A: • The values provided in the question are:-      i) pH of NaOH solution = 11.50    • We need to…

Q: Calculate the pH of a 0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K.

A: Given  0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K. pH has to be determined for…

Q: Calculate the hydroxide ion concentration of a solution with pH = 6,4.

A: pH of solution is 6.4 We need to determine [OH-]

Q: Calculate the pH of a solution that has a 0.0025 M [H3O] +

A: PH= -log[ H3O +] NEGATIVE LOHARITHAM OF HYDRONIUM ION CONCENTRATION

Q: Calculate the hydroxide ion concentration of a solution with a pH of 12.65.

A: Given :- pH of solution = 12.65  To calculate :- hydroxide ion concentration i.e. [OH-]

Q: Calculate the pH of a 0.55 M solution.

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Q: Determine [OH-] and pH of a solution that is 0.140 M in F- .

A: Given, concentration of solution with F- is 0.140M.The reaction of fluoride ion with water can be…

Q: solution has a pH = 11.4.   Calculate [H+]                              Calculate [OH-]…

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Q: Calculate the pH and the pOH of the solution at 25 °C.

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Q: The pH of a solution is 8.76. Calculate the hydrogen ion concentration of this solution in mol/L?…

A: pH + pOH = 14 pH = -log[H+] pOH = -log[OH-]

Q: A solution of H2S had a pH of 10.01. What was the [OH-]?

A:

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.