What is the [H;O *] in a solution that has a [OH ]= 2.5 x 10 8 M? A) 1.0 x 10 6 M B 2.5 x 10 22 M 7.61 M D 1.30 x 10 M 4.0 x 10 7 M E.

Q: A solution has a [H3O+] of 1 × 10−3 M. What is the [OH−] of the solution?  A)11 M  B)14 M  C)1 ×…

A: Given : [H3O+] = 1 × 10−3 M.            =10−3 M.

Q: A solution of Mg(OH)2 was found to have a pH of 12.64. Determine the initial concentration of the…

A:

Q: An aqueous solution contains a [H3O+] that is 1.0 × 10–3 M. What is the [OH–] of this solution?

A: Given :-  [H3O+] = 1.0 × 10–3 M  To calculate :- [OH-]

Q: Which of the following would be considered a neutralization reaction? O HCI + H20 → H3O+ + CI O Al +…

A: Answer

Q: 5) What is the pH of a 0.250 M HF solution? The Ka of HF is 3.5 X 104. (2.03) HF (aq) + H2O (1) A…

A: We will calculate pH

Q: Be sure to answer all parts.Calculate the concentration of OH− ions in a HCl solution whose hydrogen…

A: Concentration of OH- can be determined using given equation,

Q: What is the approximate pH of a 0.5 M solution of NaOH? A O to 1 3 to 4 C 7 to 8 13 to 14

A:

Q: The OH- ion concentration of a blood sample is 2.5 x 10-7 What is the pH of the blood?   40 40 40…

A: Concept introduction- pH - pH is defined as negative logarithm to the base 10 of H+ ion…

Q: What is the pOH of a 6.0 x 10-7 M aqueous solution of HCl? a.5.2 b.7.8 c.6.2 d.8.9

A: Hydronium ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: What is the pOH of 2x103 M HCI solution? О А. 6.2 о В. 11.3 О С. 7.0 O D. 2.7

A: 2 × 10-3 M HCl solution is considered.

Q: 9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? d. 3.2…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: HBr OH

A: The given reaction is the conversion of tertiary alcohol with HX acid to the alkyl halide.…

Q: 7) What is the pOH of a solution with a pH of 3.7? A) 14.0 B) 2.5 C) 10.3 D) 0.115 E) 0.25

A:

Q: what is the total concentration of H+ ions in ann HCL 0.025 M solution?

A: What is the total concentration of H+ ions in an HCl of  0.025 M solution?

Q: What is the pOH of a 0.030 M solution of barium hydroxide? A)12.78 B) 12.48 C) 1.52 D) 1.22 E)…

A: Given  0.030 M solution of barium hydroxide

Q: The [OH-] concentration of a solution is 5.67 x 10-8 M. The solution is O basic O neutral O acidic

A: Answer:- Given [OH-] concentration of solution is 5.67×10-8 M  We know that  poH = -log[OH-] poH =…

Q: 1. Find the pH of a solution having H+ concentration of 3.52 x 10-11. 2. What is the pH of a…

A:

Q: A solution has [H⁺] = 4.9 10⁻³ M. The [OH⁻] in this solution is A) 1.0 10⁻¹⁴ M B) 4.9 10⁻¹¹ M C) 4.9…

A: Given is, [H⁺] = 4.9 ×10⁻³ M

Q: what is the ph of a solution with (H3O+) = 2.8 *10^-9 M? a. -8.6 b. -5.4 c. 3.6 *10 ^-6 d. 5.4…

A: pH = -log(H3O+)

Q: 2) Calculate the pH corresponding to each of the following [H ] concentrations: a) 2.3 x 10° M b)…

A:

Q: 8. The normal pH of human blood ranges from 7.35 to 7.45. Calculate the concentrations of H3O* and…

A: Given,  pH  = 7.45 [H3O+] = 10-pH = 10-7.45 = 3.55×10-8 M   [OH-] = 10-14/[H3O+]  = 2.82 × 10-7 M

Q: What is the (OH] in a solution that has a [H30) = 1 × 10°2 m? 1x 10-10 M 1x 106 M B. oc* 10-8 M IC.…

A:

Q: What is the [H+] concentration of a solution with a pOH of 5?

A:

Q: An aqueous solution has a hydrogen ion concentration of 1×10-9 M   (10 -9 M). (1) What is the…

A: The given hydrogen ion concentration is 1 x 10 -9 M. The relation between hydrogen ion concentration…

Q: What is the pOH of a solution if the H+ concentration is 3.8 x 10^-8?

A:

Q: What is the pOH value when the solutions hydroxide concentration is 1.0 x 10 M? O a) -8 b) 8 c) 6 d)…

A: According to Bronsted-Lowry concept a base gives hydroxide ion. From the hydroxide ion concentration…

Q: What is the OH– concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 ´ 10–14)

A: Acid-base equilibrium.

Q: What is the pH of a 0.150 M NH4Cl solution? Kb of NH3 = 1.76 × 10−5

A: Given, Concentration of NH4Cl solution (C) = 0.150 M Kb for NH3 = 1.76 × 10-5 pH of a NH4Cl solution…

Q: ii) What is the pH value of the solution that has 0.025 M H* ion? (eH = -log[H*])

A: Concentration is given in the question

Q: If you have a solution with a [H+] of 6.87x10- M, what is the pH of the same solution? 9.16 6.16 O…

A: pH = - log [H+] pH = - log (6.87 x 10-5) pH = -[ log (6.87) + log (10-5)] pH = -[0.837 + (-5)] pH =…

Q: What is the [HF] in a solution with a pOH of 12.5? the answer is not listed 3.16 x 10:13 M 0.0316 M…

A:

Q: Calculate [H3O+] when pOH is 8.90  Calculate the pH of an NaOH solution where [OH-] = 4.6 x 10-5

A: Concentration of H3O+ can be calculated as follows:

Q: Beaker B: 50% dissociation volt What type of solution would you expect to be in Beaker B and why? OA…

A: A acid/base is weak because it's dissociation in water is very less i.e.5-7%  A acid/base is strong…

Q: What is the pH of a 0.015 M aqueous solution of barium hydroxide? A) 12.18 B) 12.35 C) 1.82 D)…

A:

Q: What is the pOH of a solution that has ​[OH^-] = 2.7E-4 M

A: pOH can be expressed as -log[OH-]. It is used to represent basicity of a solution. If the pOH value…

Q: What is the pOH for a solution that has 1.5 mol of HF dissolved in 2.0 L of water? Ka HF = 6.6 x…

A: Given  Ka HF = 6.6 x 10-4  and  1.5 mol of HF dissolved in 2.0 L of water.  pOH of the solution has…

Q: The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? 4.2 x…

A: Given that, pH =4.80 Then, [OH-] = ?

Q: Which of the following is the pH value of an aqueous solution with an OH- concentration of 0.00250…

A: pH or power of hydrogen is defined as the negative logarithm of hydrogen ion concentration present…

Q: Determin the pOH for a 1650 mL solution of 3.00 g of Mg(OH)2

A: Given that:                        Volume of the solution = 1650 ml = 1.65 L           Mass of…

Q: 4. The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood? pOH…

A: In this question, we have to first find out the pOH of the blood then, we can find pH from it.

Q: The pH of a solution is 9.67. Calculate the hydrogen ion concentration in the solution. [H*] = 2.1 x…

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

Q: What is the OH` ion concentration in a 5.2 ´ 10-4 M HNO3 solution? 1.0 x 10-4 M 1.0 x 10-7 M Zero…

A: As we know HNO3 being a strong acid , is completely ionised/dissolved in solution  the reaction is…

Q: What is the pH of a 0.010 M solution of HF?(a) 1.58 (b) 2.10 (c) 2.30 (d) 2.58 (e) 2.64

A: HF is a weak acid with dissociation constant Ka = 6.8 X 10-4 The dissociation reaction of HF is  HF…

Q: If a solution has a pOH of 5.2 the [OH-] of the solution is 6 x 10 M b. 6.3 x 10 M 1.58 x 105 M d. 2…

A: Given: pOH of the solution = 5.2

Q: aqueous solution the [H*] is 1.4 x 104M. The [OH] in the same solution is A) 1.4 x 10-2 M B) 1.4 x…

A: The relation between the hydroxide ion concentration and the hydrogen ion contraction is given as…

Q: What is the pOH of an aqueous solution of 7.72×10-2 M hydrobromic acid?

A:

Q: Assume that vinegar is a 0.852 M solution of acetic acid (HC 2 H 3 O 2 ) in waterWhat volume of…

A: Molarity is the concentration term. It is the number of moles of solute per liter Volume of…

Q: The pOH of a solution is 9.05. What is the H* concentration in the solution?

A: [OH-] = 10-pOH  [H+].[OH-] = 10-14  [H+] = 10-14/ [OH-]

Q: In a certain acidic solution at 25 °C, [H+] is 100 times greaterthan [OH-]. What is the value for…

A: pH and pOH  are related as follows:

Q: What is the [H*] in a 0.01 M Ba(OH)2 solution? A. 1 x 10-2 M B. 5 x 10-13 M. C. 1 x 10-7 M D. 1 x…

A: "Since you have asked multiple question, we will solve the first question for you. If you want any…

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.