weak base is 2.5 × 10-6, what is the pH of a 0.23 M solution of this base?

Q: If the hydronium ion concentration of a weak acid is 6.32 x 10 M what is the pH?

A: Given :- concentration of hydronium ion = 6.32 x 10-4 M  To calculate :- pH of the solution

Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

A:

Q: The K, of a certain base is 4.4x107. What is the pH of a 0.30-M solution of this base?

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Q: what is the Ph of [H3O+] = 2.5x10-5

A: pH of any solution is given by  pH = -log[H3O+ ] where [H3O+ ] = concentration of H3O+ ions

Q: The pH of an acidic solution is 2.19. What is [OH]?

A: The question is best on the concepts of PH. we have to calculate hydroxide Ion concentration.

Q: What is the pH of a solution that has [H3O*]= 4.5x10-³ M?

A:

Q: A solution of 0.00100 M HCI has a pH of: (HCl is a strong acid and dissociates completely in…

A: Given that, Concentration of HCl acid = 0.00100 M Since, HCl is a strong acid, it completely ionised…

Q: Calculate the ph of the [OH-] = 2x10^-3 M.

A: We have to calculate the pH of given solution.

Q: If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution, the pH of the…

A:

Q: 8. What is the pH of a cup of coffee that has a [OH-] of 1.200 x 10-10?

A: Detail mathematical calculation is shown below

Q: What is the pH of a solution if the concentration of H 3 O^ + is 5.6 * 10 ^ - 5 M?

A: Given data contains, Concentration of H3O+ is 5.6×10-5.

Q: If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?

A: From the relation, pOH is calculated as,

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

A:

Q: 10. What is the pH of a 0.4M ammonia solution? The ionization constant of ammonia is 1.8 X 10.

A: Given: Concentration of ammonia solution = 0.4 M Kb of ammonia = 1.8×10-5

Q: A solution that has a hydrogen ion concentration equal to 3.52 x 10-3 has a pH = _____________?

A:

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

A:

Q: A solution contains [OH-] = 4.88 x 10-6 M. What is the pH of the solution?

A: Given   The concentration of OH- is 4.88×10-6 M.

Q: What is the pH of 2.9x10 M

A:

Q: calculate ph of 7*10^-3 M aqueous solution of Ca(OH)2 at 25 degrees

A:

Q: What is the pH of a 7.7 x 10® M KOH solution?

A: Here ,the concentration of KOH is less , so we can not neglect the concentration oh OH- comes from…

Q: What is the pH of a 1.00 molar solution of NH4Cl(aq)? The Kb for NH3 = 1.8 × 10–5 .

A: Ammonium chloride dissociates completely into ammonium and chloride ions. The ammonium ion is the…

Q: What is the molar concentration of a weak acid [HA], if the ka = 6.34 x 105 and the [H*] = 9.77 x…

A: Dissociation of weak acid :   HA  ⇌H+ + A-

Q: If the pH of a solution is 6.7, the [H*]= 2 x 107 5 x 10 6 8 x 107 5 x 107 O O O O

A: Acids are the chemical compounds which donate proton, H+ in the solution while base is a chemical…

Q: If the K, of a weak base is 2.7 x 10, what is the pH of a 0.30 M solution of this base?

A: Solution Ph may be a live of however acidic or basic is AN solution.It is measured in terms of…

Q: Which of the following is the weakest base? O fluoride anion, F2 O bromide anion, Br? O chloride…

A:

Q: What is the pH of the solution if the hydroxide ion concentration is 1.0 x 10-6? 4 8. 10

A:

Q: How does the hydronium ion concentration, (H3O+) change when the pH of a solution is lowered from…

A: pH = -log[H3O+]  log[H3O+] = -pH  so, [H3O+] = 10-pH

Q: The pH of a solution for which [OH–] = 1.0 x10–6 is

A: Given:

Q: What is the pH of the following solutions? [OH-] = 9.1 × 10-3 M

A: We can only Calculate the pH of solution if we know the Hydrogen ion concentration of solution. To…

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

A:

Q: 2. Complete the following table: [H;O*] [OH] pH Solution is acidic, basic or neutral 4.56 X 102 3.5…

A: In the given problem we are required to complete the table in which we have to calculate the pH,…

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

A:

Q: What is the pH of a solution that has a [OH] = 3.3 x 10-³ M

A: pH is the negative logarithm of the concentration of H+. pOH is the negative logarithm of the…

Q: What is the pH of an aqueous solution with a hydroxide ion concentration of 4.20 x 10-4 M?

A:

Q: What is the pH of the following solutions? [H+] = 1.5 × 10-3 M ▪ [H+] = 8.7 × 10-12 M %3D [OH-] =…

A: The solutions are given below -

Q: A solution has an OH⁻ concentration of 1.3 x 10⁻⁴. What is the pH of the solution at 25°C?

A: pH = -log [H+] [H+][OH-] = 1 x 10-14     at 25°C

Q: 11. If the [H+] is 1 x 10 ^-3 . What is the pH of the solution?

A: Interpretation -  To determine the pH of the solution when concentration of [ H+ ] is given as 1 ×…

Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

A:

Q: Lemon juice has a pH of about 2. What [H3O+] is this?

A: Given that the pH of lemon juice is 2. To calculate the concentration of H3O+ ions in the lemon…

Q: What is the pH of a 6.9 × 10⁻⁶ M KOH solution?

A: Use formula POH= -log(OH-) PH+POH=14 PH= 8.84

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: (6)  Is the salt C2H5NH3Cl acidic, basic, or neutral?                            What is the pH of…

A:

Q: 8. Calculate the pH of NaOH(aq) to the nearest hundredth.

A: Given data : Molarity of NaOH = 0.20 M

Q: What is the pH of a solution if the concentration of H+ is 5.3x 10^-9

A: pH of solution = ? H+ = 5.3 × 10-9  We know that, pH = - log [H+]

Q: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: calculate the ph of [OH-]=8.7x10-6M

A: We have to calculate the pH of solution having given concentration.

Q: A certain weak base has a Kb of 8.60×10−7M. What concentration of this base will produce a pH of…

A:

Q: If the hydronium ion concentration is 2.5 x 10^-4, what is the pH ? __ Is this am acid or base ?

A: The concentration of hydronium ion (H3O+] = 2.5 × 10-4  pH = ?  This is an acid or base ?

Q: Calculate the pH of a solution with an H+1 concentration of 1.80 x10-2 M.

A: pH of any solution is given by  pH = -log[H+ ] where [H+ ] = concentration of H+ ions

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.