What is the concentration of hydrogen ions in a solution if it's [OH^-] is 2.5 x 10^-10M ?

Q: Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO(aq) +…

A: According to the Law of conservation of mass " all atoms of different elements must be equal on both…

Q: If the pOH of a solution is 12.67, what is the concentration of the OH-?

A: pOH = 12.67

Q: Why is ammonia described as a Brønsted-Lowry base andnot an Arrhenius base?

A: According to  Arrhenius base theory bases are hydroxide ion donors.

Q: What is the [OH-] if the [H+] concentration is 3.1x10^-4 Molar?

A: The concentration of H+ ions is 3.1×10-4 M. The relationship between the concentration of H+ ions…

Q: In a sample of lemon juice, H+ concentration is 3.8 x 10-4 M. What is the pH?

A: we know pH = −log [H+] where   [H+]  = concentration of H+

Q: According to the Brønsted-Lowry theory, label each of the following as an acid or a base. (a) HNO;…

A: Bronsted-Lowry theory: This theory basically focuses on proton transfer.. Bronsted-Lowry acid: It is…

Q: a solution has a concentration of OH- =4.0x10-5 M. what are the concentration of H3O+ and the pH of…

A: pH of a solution can be defined as negative of logarithm of concentration of hydronium ions

Q: Which of the following is the formula for a weak acid? О А. НF B. HCIO4 C. H2SO4 O D. HNO3

A: Weak acid  is partially  dissociate into its  ion in aqeous  solution  (I.e. water) . And strong…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.7 × 10⁻³. What is [H⁺]?

A:

Q: If H+ is equal to 6.9x10^-5, what are the values of pH, POH, and OH-?

A: Given - [H+ ] =6.9*10-5 We have to determine pH, pOH and concentration of OH-.

Q: An aqueous HCl solution has a proton concentration equal to 6.00 mol/L. The HCl concentration in…

A: Molarity is defined as the number of moles per liter of the solution. It is expressed as mol/L.

Q: If a solution has a hydroxide ion concentration of 8.57x101-4, what is the concentration of…

A:

Q: A solution has [OH¯] = 4.0 × 10-. What is the value of [H*] for the solution?

A: Given :- [OH-] = 4.0 × 10-8  To calculate :- [H+]

Q: A solution of HCl has a ph of 2.3. If so what is [OH-]?

A:

Q: For a given aqueous solution if [H+]=1.0x10^-9 M, what is [OH-]

A: Concentration of [H+]=1.0x10^-9 M in aq.solution. Concentration of [OH-] = ? Formula: Ionic…

Q: [References) A solution of hydrochloric acid is 1.6 x 10-4 M HC1. What is the hydronium-ion…

A:

Q: 101 strong bases - Google Search Question 2 of 16 Complete the balanced neutralization equation for…

A: This is a acid base reaction . HBr is acid and LiOH is base . Acid gives H+ and Base gives OH-

Q: The H⁺ concentration in an aqueous solution at 25 °C is 9.3 × 10⁻⁶. What is [OH⁻]?

A: • The values provided in the question are:-      i) Hydrogen ion concentration of a solution, H+ =…

Q: Assuming complete dissociation, what is the pH of a 0.348 M Ba(OH), solution? (Round your answer to…

A: Given  Concentration of Ba(OH)2  =  0.348 M  PH = ?

Q: What is the pH of a 1.5x10-7 NaOH solution?

A: Given , Solution is NaOH Molarity = 1.5×10-7  { I am considering the the solution expressed in…

Q: The H⁺ concentration in an aqueous solution at 25 °C is 2.9 × 10⁻⁶. What is [OH⁻]?

A: For an aqueous solution, The H⁺ concentration, [H⁺]=2.9 × 10⁻⁶ M The concentration of OH⁻ ions has…

Q: A solution has an [H_O*] = 8.25 x 109. Calculate each of the following values for this solution [OH]…

A: We have given that [H3O+] = 8.25 × 10-9 We Know that                     [H3O+] [OH-] = 10-14…

Q: if the concentration of OH- in an aqueous solution is 1.4 x10^-7 M, the concentration of H3O+ is…

A: Given;

Q: If the (H*) in a solution is 6.23 x 10$ M. What is the pH?

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: Hydrochloric acid (HCl) is a strong acid, meaning it is 100% ionized in solution. What is the [H+]…

A: Given,  [HCl = 2.0×10−3 M What is the [H+] and the [OH−] in a solution = ?

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

A:

Q: An acid solution has a greater amount of H3O+ or OH- ions? (Which one)

A:

Q: What is the pOH of an aqueous solution of 0.144 M hydrochloric acid? pOH =

A: In this question, we have to determine the pOH of aqueous solution of 0.144 M hydrochloric acid. pOH…

Q: If a solution has [OH-] = 3.64 x 10^-7, what is the hydronium ion concentration?

A:

Q: What is the pH of a HCI solution with a concentration of 6 x 104 M?

A: pH= -log [H^+]

Q: The H⁺ concentration in an aqueous solution at 25 °C is 6.7 × 10⁻⁴. What is [OH⁻]?

A:

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

A:

Q: 3. An aqueous HCl solution has a proton concentration equal to 6.00 mol/L.The HCl concentration in…

A: The answer to the following question is :

Q: For a solution with a hydroxide (OH-) concentration of 5.0 x 10-5 M, what is the concentration of…

A:

Q: An acid increases the concentration of H+ in aqueous solution, and a base increases the…

A: Acids are defined as one which releases protons to the solution or accepts a pair of electrons.…

Q: 4. What would the hydroxide ion concentration be if the hydrogen ion concentration was 1 x 10 M?

A: Given data for this, [H+] = 1×10-5 M

Q: A beverage has a hydronium-ion concentration equal to 3.3  10-3 M. What is the pH of this beverage?

A: [ H3O+] = 3.3 × 10^(-3) = [H+]  pH  = - log [H+]

Q: b. In question 5a, what is the molar concentration of all ions in solution? [K* ] = M [SO,? ] = M

A: The molar concentration of all the ions of a salt can be obtained knowing the molarity of the salt…

Q: -OH + HCI

A: Sequence :- Protonation of alcoholic oxygen Loss of water as leaving group Attack of nucleophile

Q: What are the concentrations of H+ and OH− in a solution of 150 mM HCl?

A: Conc. of given HCl Soln  = 150 mM  (Since 1 M = 1000mM )  = 0.15 M   H+ + Cl- ---> HCl  As we can…

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.7 × 10⁻⁴. What is [OH⁻]?

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: A solution has a hydrogen ion concentration of 1 x 10^6 M. What is the pH?

A: The negative logarithm of concentration of hydrogen ion is known as pH. pH = – log [H+]

Q: Q2:a) 1. What is the pOH of a 0.10 M NaF solution? K, HF = 7.ZX 10

A: The question is based on the concept of PH calculations. sodium fluoride is the salt of strong base…

Q: Write the formula of the conjugate acid for the following base. OH−

A: Conjugate acids and bases are Bronsted-Lowry acid and base pairs, determined by which species gains…

Q: The concentration of OH- ions in a particular household ammonia cleaning solution is 0.075M. What is…

A:

Q: A solution of hydroiodic acid has a concentration of 2.00x10-2 M. What is the pH of this solution?…

A: Given: Concentration of hydroiodic acid i.e. HI = 2.00 × 10-2 M.

Q: Which of the following is a weak base? А. CH:NH, В. HNO, C. HCl D. NAOH

A: Weak Base: Bases that has little affinity towards protons. Weak base forms stronger conjugated acid.…

Q: The H⁺ concentration in an aqueous solution at 25 °C is 5.9 × 10⁻⁴. What is [OH⁻]?

A: Given- The H⁺ concentration in an aqueous solution at 25 °C is 6.7 × 10⁻⁶.

Q: In a solution of Ba(OH)2, if the concentration of the hydroxide ion is 0.45 M, what is the…

A: Barium hydroxide is a strong base which undergoes complete dissociation in aqueous solution giving…

Q: A solution has a pOH of 2.00. What is the [H+] and [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.