What is the pH of a 0.0000100 M solution of CsOH?

Q: (b) What are [H3O+], [OH -], and pH in a solution with a pOH of 4.19?

A: Since we know that pH + pOH = 14  => pH for the above case = 14 - pOH = 14 - 4.19 = 9.81

Q: The pH of a chemical solution is given by theformula pH = - log10 [H+ ] where [H+ ] is the…

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

Q: The pH of a 0.0059 M solution of Ca(OH)₂ is

A: The objective of the question is to calculate the pH of a 0.0059 M solution of Ca(OH)₂. The pH of a…

Q: Calculate the pH of the solution.  Assume 5.0 L of solution. You must identify the type of solution…

A: Given that: volume of solution = 5 L moles of NH3 = 0.190  moles of HCl = 0.120  Kb(NH3) = 1.8 x…

Q: What is the pH of a 0.0023 mol/L solution of nitric acid? The answer should be to the proper number…

A: pH of the solution is calculated as  pH = – log[H+] Given that [HNO3] = 0.0023 mol/L

Q: The pH of a 0.0069 M solution of HNO₃ is?

A: The objective of the question is to calculate the pH of a 0.0069 M solution of HNO3. HNO3 is a…

Q: How many moles of NH3 must be dissolved in water to give 622.4 mL of solution with a pH of 11.08? Ko…

A: Given -> Volume of solution= 622.4 ml = 0.6224 L (1L = 1000ml ) pH = 11.08  Kb = 1.8 × 10-5

Q: Calculate the pH of a 0.170 M solution of potassium nitrite, KNO₂. pH =

A: Given that, [KNO2] = 0.170 M =C (LET)  pH = ?

Q: What is the pH of a 0.45 mol/L solution of hydrobromic acid? The answer should be to the proper…

A:

Q: What is the pH of a 7.041 x 10^-6 M HCIO4 solution?

A: Given , concentration of acid solution = 7.041 x 10^-6 M   That means,  [H+] = 7.041 x 10^-6 M

Q: Calculate the pH of a 0.525M solution of hypochlorous acid, HCIO. %3D

A:

Q: What is the pH of a 0.00535 M solution of NaOH?

A: Number of moles of solute present in one litre of Solution is called Molality (M)  Units: mol/L  pH…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.23 M solution…

A: The PH of diprotic acid can be calculated as follows

Q: At 25°C, calculate the pH of a 0.426 M solution of the salt KNO2. (Ka (HNO2) = 4.50 × 10−4 ).

A:

Q: Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH…

A: pH of the solution is equal to the negative logarithm of the concentration of hydronium ions H3O+.…

Q: 6) What is the pH and pOH of a solution with a [OH] of 7.79 X 10* M? Is the solution acidic, basic…

A:

Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH can be calculated as follows

Q: The pH of vinegar is about 2.5. Calculate the [H3O+] for vinegar.Calculate the [OH−] for…

A: The objective of the question is to calculate the concentration of hydronium ions [H3O+], hydroxide…

Q: What is the pH of a 0.800 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Information about the question

Q: Calculate the pH of a 5.714 M solution of NaHS

A: Given Concentration of NaHS is 5.714 M To find pH of the given solution

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

A:

Q: The pH of a 0.0070 M solution of HNO₃ is

A:

Q: The ph of vinegar is 2.7. Calculate the hydronium ion concentratio

A: Here given PH of vinegar = 2.7 We have to calculate conentration of hydronium ion .

Q: 6a) Write the hydrolysis reaction of hypochlorous acid Clearly identify the acid, base, conjugate…

A: Given data:Concentration of solution of acid =0.050 MDetermine the hydrolysis reaction of…

Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: what is the pH of a 0.00761 molar solution of HNO3?

A: Nitric acid is a strong acid that dissociates completely in aqueous solution.

Q: The pH of the 0.50 M solution of HA is 1.92. What is [HA]?

A: Answer:pH is equal to negative of logarithm of hydrogen ion concentration in solution, so,

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.45 M solution…

A: The question is based on the concept of equilibrium. we have determine the pH of the given diprotic…

Q: The pH of an acidic solution is 3.37. What is [H⁺]?

A:

Q: Which of the following can be classified as a Lewis base? BH3 O I only II, III, and IV O I and II O…

A: Lewis bases are those compounds which has lone pair of electrons to donate.  Lewis acids are those…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: The pH of a 0.0041 M solution of HNO₃ is

A:

Q: The pH of a 0.0046 M solution of HNO₃ is

A: The pH of the solution is = 2.34

Q: The pH of a 0.0052 M solution of HNO₃ is

A: Nitric acid (HNO3) is strong acid hence it dissociated fully in aqueous solution

Q: Find the pH of a 0.043 M HClO4 solution.

A: Given :- concentration of HClO4 = 0.043 M  To calculate :- pH of the solution

Q: What is the pH of a 0.0610 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

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.