Determine the pH, OH -, H3O+ and ph for a solution made by dissolving 121 mg of HCl in 555 mL of water

Q: The pH scale measures the number of H+ ions in a solution. If there are a lot of H+ 1ons, is the pH…

A: High

Q: The pH of a basic solution is 12.17. What is [H]? M 3 4 6. C 7 8 +/- x 100

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Q: Write an equation showing that rubidium hydroxide (RbOHRbOH) acts as an Arrhenius base in water.

A: Arrhenius base is defined as they give OH-in aqueous medium.

Q: What is the concentration of H3O+, in M, of a solution with a pH of 1.11?

A: Given :  pH of Solution = 1.11 [ H3O+ ] = ? We know the following formula  pH = - log[ H3O+ ]

Q: Which of the following solutions has the highest pH: (a) 0.40 M HCOOH, (b) 0.40 M HCIO4, (c) 0.40 M…

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Q: At 25 °C, how many dissociated OH ions are there in 1285 mL of an aqueous solution whose pH is 1.23?…

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Q: Calculate [H3O+], [OH-], pH, and pOH for the following solutions. Assuming complete dissociation for…

A: From the given Species , first concentration of H3O+ or OH- is calculated based on their nature.…

Q: The hydronium ion concentration of an aqueous solution of 0.43 M formic acid, HCOOH is  [H3O+] =…

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Q: In the reaction SnCl4 + 2Cl- = (SnCl6)2- which acts as the Lewis base?

A: We have to identify the Lewis base for the following given reaction SnCl4 + 2Cl- = (SnCl6)2- as…

Q: Without using a calculator, determine the pH and pOH of each solution. Rank the solutions from most…

A: The formulae required for the calculation pH = -log [H+] pOH = -log [OH-] pH + pOH = 14 pH = 14 –…

Q: Acids and Bases: Classify the following solution as acidic, basic, neutral, or neither. [Na+] =…

A: Given : [Na+ ] = 0.000 M [OH- ] = 1.0 X 10-7 M And [H3O+ ] = 1.0 X 10-7 M

Q: Find the [OH-] and pH of a 0.010 M Ba(OH)2 solution.

A: Given, 0.010 M Ba(OH)2

Q: 5. In a NaOH solution [OH2] is 2.9 x 10-24 M. Calculate the pH of the solution.

A: NaOH is  a strong base so, it completely dissociate into its ions in aqueous solution. NaOH (aq)…

Q: Phthalic acid (H, C,H,O,) is a diprotic acid with K1.12 x 10 and K- 3,90 x 10, Determine the pH of…

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Q: Show complete calculations Calculate the pOH, H3O+, OH- if the pH is: 1. pH = 3.75 2. pH = 2.5

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Q: The base protonation constant K, of ammonia (NH,) is 1.8 x 10 °. Calculate the pH of a 0.86 M…

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Q: What is t pH of an aqueous solution that is 2.7 x 10-3 M HCl

A: Given, Concentration of HCl solution = [HCl] = 2.7 x 10-3 M pH of the solution = ? Note:  HCl is a…

Q: Convert 0.035 M OH- concentration to pH value (in aqueous solutions).

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Q: Q1- SOLVE mathematically, then choose the correct answers: (42 marks) 1- Calculate the pH of…

A: Given,  Volume of CH3COOH = 100 mL Molarity of CH3COOH = 0.28 M = 0.28 mol/L  Volume of NaOH = 50 mL…

Q: Calculate the [H*], pH, and pOH in each of the following solutions in which the hydroxide ion…

A: The given question contains more than three sub-parts, so answer to first three sub-parts have been…

Q: Calculate the pH of the following acid or base: 1. 3.6 x 10-7 M HNO3 2. 2.0 x 10-4 M NaOH

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Q: Determine the pH of a 0.200 M benzoic acid at 25°C. Benzoic acid is a weak monoprotic acid, with the…

A: Benzoic acid a weak monobasic acid with Ka of 6.3 x 10-5 at 25 degree Celsius.

Q: The base protonation constant K, of ammonia (NH,) is 1.8 x 10. Calculate the pH of a 0.15 M solution…

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

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Q: What is the ph of a solution in which the hydrogen ion concentration is 1.0x10^-5 m?

A: The pH of a solution is defined as the negative logarithm of the concentration of Hydrogen ion, that…

Q: Write the formula for the conjugate base of each acid.a. HCl b. H2SO3 c. HCHO2 d. HF

A: A conjugate base is formed when a proton is removed from an acid.

Q: Calculate [H3O+] when given the [OH-] in each of the following aqueous solutions and classify the…

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Q: classify the solution as acidic, basic, or neutral. [H3O*] [OH] pH РОН Classification 6.3x 104 2.5x…

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Q: At 25 °C, how many dissociated OH ions are there in 1221 mL of an aqueous solution whose pH is 1.26?…

A: pH of an aqueous solution is given 1.26. we know,  pH + pOH=14 Or, 1.26+ pOH=14 Or, pOH=…

Q: Which of the following is a conjugate acid-base pair? A) OH-, H2O B) NH3, OH- C) OH¯, NH.* D) H:O,…

A: According to Bronsted-Lowry ,a conjugate acid -base pair consists of two substances that only…

Q: Write the formula for the conjugate base of HCN.

A: A conjugate base of an acid can be drawn by reducing one proton from it and putting a negative…

Q: a) Write the formula for the conjugate base of HPO, -2 b) Write the formula for the conjugate acid…

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Q: 1) Indicate whether each solution is acidic, basic, or neutral: -4 a) 2 x 10 M OH b) 6 x 10 M H -10

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Calculate[OH-] if [H3O+] = 5.2 x 10-11M. Indicate whether the solutions is acidic, basic, or…

A: The term pH of the solution is a measure of the acidity or the basicity of a given solution. More…

Q: The pOH of an aqueous solution of 0.371 M dimethylamine (a weak base with the formula (CH2),NH) is

A: Given: Concentration of dimethylamine = 0.371 M Kb of = 5.9×10-4

Q: Consider the following acid-base reaction: HSO, + HF 2 H,SO, + F Based off of the given equation,…

A: Introduction : We have to tell about bronsted lowry acids and bronsted lowry base .

Q: What is the H 3O + concentration in lemon juice that has a pH of about 2? Classify the solution as…

A: The pH is a method that helps in the determination of the acidity and basicity of the given…

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 1.10 × 10-º M. pH

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Q: Consider 0.25 M solutions of the following salts: NaCl, RbOCl, RbOCl, Kl, Ba(ClO4)2, and NH4NO3. For…

A: Interpretation: To determine whether 0.25 M solutions of the salts NaCl, RbOCl, Kl, Ba(ClO4)2, and…

Q: If the [OH^-] of a solution is 1 x 10^-6M, what is the concentration of the hydronium ion ? __ Is…

A: Given : [OH-] = 1 x 10^-6M

Q: Calculate the [H+], [OH-], pH and pOH of a solution that contains 1.35g of aluminum hydroxide…

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Q: Determine the pH of a 0.741 M OH- solution at 25°C.

A: • The values provided in the question are:-     i) Hydroxide ion concentration of a solution, [OH-]…

Q: HCl(aq) + H2O(l) ⇌ Cl-(aq) + H3O+(aq) Identify the acid, base, conjugate acid, and conjugate base

A: Acid: The molecule contains hydrogen atom that molecule donate Hydrogen atom  to any other…

Q: Calculate the [OH-] in each of the following solutions, and indicate whether the solution is acidic,…

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Q: What is the [OH-] , [H+] and pH of a solution containing 0.00086M KOH

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: Calculate the pH of the solution. Assume 5.0 L of solution. You must identify the type of solution…

A: Answer is explained below. Given that, solution contains 0.190 moles NH3 & 0.120 moles HCl.…

Q: Classify each as a strong acid, weak acid, strong base, or weak base. a. HASO, b. Sr (OH)2 C. HIO d.…

A: The species that increase the concentration of hydrogen ions or hydronium in an aqueous solution act…

Q: The base protonation constant K, of ammonia (NH,) is 1.8 x 10. Calculate the pH of a 1.2 M solution…

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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.