What is the hydroxide concentration, [OH-], of a pH 5.26 solution?

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 with [OH-]=2.2 x 10^-7M?

A: In this question, we will determined the pH of the basic solution. So, first we need to determine…

Q: What is the molar concentration of H3O+ in an aqueous solution with a concentration of OH-  that…

A: We have to calculate the molar concentration of H3O+ in an aqueous solution with a concentration of…

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

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: 6. OH- concentration is 1.233x10(-7). What is the pH? 8.09 5.09 6.09 7.09

A: PH = -log [H+] POH= - log [OH-] Given [oH-]= 1.233×10-7

Q: What is the [H3O+] for a solution with a [OH-] of 7.79 X 10-6 M? Is the solution acidic, basic or…

A: The solution which have: pH > 7 basic pH = 7 neutral pH < 7 acidic

Q: What is the pH of lemon juice with a [H+] of 2.0x10-3?

A:

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: For 8.73 x 10-3 M LiOH, determine [OH-] and [H3O+]. Express your answers in moles per liter to three…

A: Lithium hydroxide is a strong electrolyte and it dossociates completely as follows:Hence the…

Q: pH

A:

Q: If the hydronium ion (H3O+) concentration of a solution is 1 x 10-11 M (at 25°C), then what is the…

A:

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

A:

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

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: 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: What is the pH of a solution of HCL in which (HCI] = 2.6 x 10 M7 (2 decimals only)

A:

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

A:

Q: In an aqueous solution the  [OH-] is 1.0 x 10- 6 M. What is the [H+]

A: At 25oC, the mathematical relation between molarities of H+ and OH- is given as: [H+][OH-]=1.0×10-14…

Q: What is the pH of a 2.5 M solution of HC1O4? pH

A:

Q: What is the hydroxide ion concentration of a solution with pOH =1.5?

A:

Q: Calculate the [H+] of a solution prepared by combining 1 L of a HC1O4 solution with pH = 2.00 and 1…

A: Given data, pH of HClO4 solution = 2.00 Volume of HClO4 = 1.0L Volume of H2SO4 = 1.0L pH of H2SO4 =…

Q: What is the original concentration of a Strontium Hydroxide Solution with a pH of 13.22?

A:

Q: if the pOH of sodium hydroxide was 12.07 what is the [H+]

A: The sum of pOH and pH is equal to 14.

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: A solution is found to have a pH of 8.3, what is the hrdroxide ion [OH-] concentration?

A: Introduction If we know the pH of any particular solution, then first [H+] is calculated then with…

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: A solution of NaOH has a pH of 9.52. What is its pOH, [H3O'], and [OH-] at 25?

A:

Q: What is the [H+] of a solution whose pOH = 2.11 ?

A:

Q: An acid (HA) dissociates as follows: HA → H+ + A minus Arrow should be interpreted as an…

A: [H+] can be calculated by using formula

Q: HCI has a pH of 3. What is the concentration [OH-]?

A:

Q: solution that shows a pH of 11.70 has a  [H+] of what?

A:

Q: What is the concentration of OH^- in a solution with a pH of 10.00

A: The objective of this question is to find the concentration of hydroxide ions (OH-) in a solution…

Q: What is the concentration of [OH] if the solution with a pH=6.9?

A: Given : pH = 6.9

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 6.7 × 10⁻⁴ M, then [OH⁻] is

A: In an aqueous solution [H₃O⁺] ×   [OH⁻]  = Kw

Q: Nitrous acid, HNO₂, has a Kₐ of 7.1X10⁻⁴. What are[H₃O⁺], [NO₂⁻], and [OH⁻] in 0.60 M HNO₂?

A: First of all we have to write the equation for nitrous acid.     HNO2+H2O⇔H3O++NO-2…

Q: What are [H*], [OH-] and pH in a solution with a pOH of 12.11 15.

A:

Q: A solution has a hydronium concentration of 7.50 x 10-5. What is the hydroxide concentration in M?

A: Given = Hydronium ion concentration (H30 +) =7.50*10-5 Hydroxide ion concentration (OH-) =?

Q: pH of a solution having OH-  concentration 10-5

A: We know that, pOH = -log[OH-]                { [OH-] is the molar concentration of OH- ion} Again,…

Q: A solution of 0.10 M HCl has a pH = 1.00, whereas a solution of 0.10 M CH3COOH has a pH = 2.88.…

A: The dissociation of HCl is represented as, HCl→H++Cl- The dissociation of acetic acid represented…

Q: Calculate the hydroxide ion concentration, [OH−][OH−], for a solution with a pH of 5.615.61.…

A:

Q: The daily output of stomach acid (gastric juice) is 1000 mL to 2000 mL. Prior to a meal, stomach…

A: Total number of moles of OH- ion present in milk of magnesia need equal number of moles of hydronium…

Q: What is the pH of a solution with [H+] = 3.51x10-5 M

A:

Q: In an aqueous solution at 25 °C, if [H₃O⁺] = 7.2 × 10⁻⁴ M, then [OH⁻] is

A: Given,[ H3 ] = 7.2 x 10-4 M at 25.0 oC

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

A: pH +pOH = 14

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.