What is the pH of a 0.000000220 M KOH solution at 25oC? Answer to three significant figures.

Q: Ka for nitrous acid, HNO2, is 4.50×10-4. Ka for benzoic acid, C6H5COOH, is 6.30×10-5. Ka for…

A: A question based on equilibrium concept that is to be accomplished.

Q: Express the pH of the solution to three decimal places. 5.69*10-2 M HNO3

A:

Q: How many grams of NH:Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16?…

A: Given that, pH of the solution = 5.16 Kb of NH3 = 1.8×10-5 Now, we have to calculate the amount of…

Q: Calculate the pH of a 0.30M solution of C5H5N. The Kb for C5H5N is 1.7×10^-9

A:

Q: Putting 10g of H2SO3 in 95mL of water will give an acid with what concentration?

A: Concentration of a solution can be calculated in terms of molarity, normality, molality, or…

Q: Determine both the H and the pH in a 0.0541 M solution of HNO3 at 25 °C? H= Type your answer here…

A: The concentration of HNO3 solution = 0.0541 M HNO3 → H+ + NO3− The concentration of H+, [H+] =…

Q: Calculate the pH of 1.055% (by mass) HCl (MM=36.46) solution. Assume density of the solution is…

A: Mass=1.055% Density =1.010 g/ml

Q: At 70 degrees celcius, Kw for pure water is 2.3x10-13 what is the pH of pure water at 70 degree?

A: Pure water dissociates as per the reaction, => H2O (l) ------> H+ (aq) + OH- (aq)…

Q: A 0.202 M solution of HX has a pH of 4.90 at 25°C. What is the value of Ka for HX? (the answer…

A:

Q: TUS V Complete the table below. Be sure each of your answer entries has the correct number of…

A:

Q: I'm a little confused on how to do the calculations. How do I do the calculations for this?…

A:

Q: Determine the [H+], pH, and pOH of a solution with [OH−]=1.6×10^−12 M at 25 °C. Round your [H+]…

A: Answer :

Q: Calculate [OH-] in each aqueous solution at 250C, and classify each solution as acidic or basic. All…

A: At 25°C Kw = [H3O+] [OH-] = 1.008 * 10-14 Or simplicity Kw = [H3O+] [OH-] = 1* 10-14 For acidic…

Q: What is the pH of a solution containing 0.453 mol L-1 HF and 0.267 mol L-1 F- ? Round your answer to…

A: Given,  [HF] = 0.453 M  [F-] = 0.267 M  What is the pH of the solution = ?

Q: What is the pOH of a .0767 M HydroIodic Acid Solution?

A: We know that, pH is the negative logarithm of hydrogen ion concentration and pOH is the negative…

Q: Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215…

A:

Q: Ascorbic acid (vitamin C, C6H;O6) is a diprotic acid (Ka1 = 8.0x10 and Ka2 = 1.6×10-12). What is the…

A:

Q: Calculate the size of the pH change when the ratio HA] changes from 10 to 1.

A: We can calculate it from dissociation constant of acid and we should do comparisons which is…

Q: The pH of a 0.60M solution of acrylic acid (HC3H3CO₂) is measured to be 2.24. Calculate the acid…

A: pH = 2.24

Q: H3PO4 is a weak polyprotic acid with K₁ = 7.2x10³, K₂= 6.3x10^-8, and K3 = 4.2x10^-13. What is the…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Please help me sort this and explain why.

A: Reaction of acid with water results to form hydronium ions. Generally, these reactions are…

Q: Calculate the [H+] and pH of a 2.35×10−4 M hydrazoic acid solution. The Ka of hydrazoic acid is…

A: We wil use concept of weak acid for H+ and pH.

Q: Complete the table below. Be sure each of your answer entries has the correct number of significant…

A: Complete the table of the given above--

Q: solution at 25°C is measured as 8.97 x 10^-5 M, what is the pH of the solution? Report answer with…

A: pH is equal to the negative logarithmic of hydrogen ion concentration

Q: Predicting the qualitative acid-base properties of salts Consider the following data on some weak…

A: To answer this question, you need to understand the concept of conjugate acid-base pairs.A conjugate…

Q: alculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic.…

A:

Q: Conside Tollowing data on some weak acids and weak bases: acid base K. K; name formula formula name…

A: The solutions given are,

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.