What is the pH of a 3.48x102 M solution of the strong acid HCIO,? HCIO4(aq) + H20(1)→ CIO4 (aq) + H3O*(aq) [HCIO4]0 = 3.48×10-2 %3D

Q: Carbonic acid, H2CO: is a diprotic acid with Ka1 = 4.3 x 107 and Ka2 = 5.6 x 10 11. What is the pH…

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Q: Calculate the concentration of HCO3 in an aqueous solution of 0.0557 M carbonic acid, H2CO3 (aq).…

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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: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.29 M solution…

A: Total H+ in the solution is X+Y. We should neglect values of X in front of number in denominator.

Q: What is the pH of a 0.0758 M solution of NH4Cl? Kb for NH3 = 1.8 × 10−5

A: NH4Cl is salt of strong acid and weak base

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.18 M solution…

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Q: 2. Phenol, CH;OH can act as an acid in an aqueous solution. The Ka of phenolis around 2.1 x 10°, and…

A: pH = -log[H+] pOH = -log[OH]  Also, pH + pOH = 14 Also Ka and Kb has a relationship  Ka × Kb = Kw

Q: choices

A: Dear student I have given answer to your question in the image format.

Q: If the K, of CGH5COOH is 6.3 x 10, what is the pH of a 0.227 M solution of NaCgH;COO? O 2.72 11.28…

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Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.14 M solution…

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Q: In the following equilibrium, identify the conjugate base of the weak acid? HA(aq) + H2O(1) A (aq) +…

A: Answer

Q: A solution of CSH5N (pyridine, Kp = 1.7 x 10 °) has a pH of 9.40. What is the [C5H5N]? O 9.3 x 1011…

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Q: What is the pH of 0.390 M HC1(aq)? O 0.41 0.390 O 13.61 O 13.59 O7.00

A: We have to predict the pH of the solution.

Q: Calculate the pH of a 0.100M solution of the weak base NH3. Kb of NH3 1.8×10. %3D 3)

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Q: 2. Which of the following is closest to the pH OF a solution containing 5 mM H,SO, ? А. 1 В. 2 С. 3…

A: The question is based on the concept of pH of the solution. it is defined as a negative logarithm of…

Q: Calculate the pH of a solution (aq., 25 oC) when 20.00 mL of 0.284 M HNO3 is mixed with 30.00 mL of…

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Q: Calculate the concentration of HCO3 In an aqueous solution of 0.2980 M carbonic acid, H₂CO3 (aq).…

A: The Answer to the following question is-

Q: Find the pH of a 0.22 M AlCl3 (aq) solution if Ka of Al3+ is 1.2 × 10–5

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Q: The ionization constant of lactic acid, CH;CH(OH)CO,H, an acid found in the blood after strenuous…

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Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

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Q: Calculate the pH of the following solutions and indicate whether they are acidic, basic, or neutral.…

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Q: Which of the following indicates the most acidic solution? A. [OH]=0.5 M B. [H] =0.3 M C. pOH = 5.9…

A: pH = - log [H+] pOH = - log [OH-]   [OH-] = 10-pOH  [H+] = 10-pH    pH + pOH = 14    pH = 7 :…

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N? (a) 4.48 (b) 8.96 (c) 9.52 (d) 9.62 (e) 9.71

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9   To solve: pH of…

Q: Phosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid has pKa2…

A: Solution                      Given that The solution will be as follows   Given the concentration…

Q: Indicate the pH of the following

A: pH = -log[H+]  pH + OH = 14

Q: Which of the following solution is the least acidic? ​A. [OH‾] = 1.5 × 10^-8 M   B. [H3O^+]…

A: (a) Given (b)

Q: The pH of a 0.100 M CH3NH2 solution is 11.80. What is the % ionization value? O 11.80% O 1.58% O…

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Q: does H2SO4 act as a strong or weak acid in water

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Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: Weak acids dissociate partially in an aqueous solution to furnish the hydrogen ions. The…

Q: What is  the pH of an (aq) solution, [OH-] = 4.6 × 10-10 M.

A: pH is equal to negative logarithm of hydrogen ions

Q: What is the pH of .242 M H2CO3 (aq)? O 6.38 О 3.50 O 10.50 O 4.12 O 5.47

A: pH is defined as negative log of concentration of H+ ions in the solution.

Q: Indicate the pH of each of the following solutions at room & show how you got your answer. (d)…

A: Given : Concentration of H2SO4 = 0.050 M

Q: What is the pH of a solution with a hydroxide concentration of 2.82x10 M? O A. 10.45 о В. 2.77 о С.…

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Q: Nitric acid, HNO3(aq), is an important industrial chemical. Large quantities are re production of…

A: Nitric acid HNO3 , is an important industrial chemical.Large quantities are required for the…

Q: In the acid-base neutralization reaction between 0.75 M HNO3 (aq) and 0.75M Ba(OH)- (aq), the acid…

A: 2:1 ratio   2 mole acid to 1 mole base

Q: Drinking water is often disinfected with Cl₂, which hy-drolyzes to form HClO, a weak acid but…

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Q: Ammonium nitrate NH4NO3 is a salt used in fertilizers and in making matches. The salt is made by the…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: 6.7

A: Here : O.35 M = C ( original concentration )  [H+] = √( Ka1 • C )  Using this formula, Calculate…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.58 M solution…

A: Since the Ka1 of H2A is >> Ka2 of H2A  Hence we can assume only the first dissociation of H2A…

Q: Phosphoric acid, H;PO,(aq), is a triprotic acid, meaning that one molecule of the acid has three…

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Q: Identify the following as acidic, basic, neutral, or amphoteric. AlCl3 _________ NaCI __________…

A: AlCl3 is Lewis acid because it has vacant orbitals. NaCl is salt ,thus it is neutral. SO2 is acidic.

Q: Calculate the hydronium ion concentration in an aqueous solution of 0.195 M carbonic acid, H,CO3…

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Q: Determine the pH and pOH of a solution at 25C with a hydronium ion, H₂O*(aq), concentration of…

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Q: Calculate the concentration of HCO3 in an aqueous solution of 0.1120 M carbonic acid, H,CO3 (aq).…

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Q: Determine the pH of a 0.450M solution of aniline hydrochloride. C,H;NH, * (aq) + H2O(1) = H3O*(aq) +…

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Q: What is the conjugate acid for HNO_2(aq)?

A: HNO2 is itself an acid, so it will form stable conjugate base by loosing its H+ ion.  Conjugate base…

Q: What is the pH of a 0.233M solution of aniline hydrochloride?           C6H5NH3+(aq)  +   H2O(l)…

A: The acid dissociation constant of anilinium is calculated as,

Q: A diprotic acid, H2A, has Ka1 = 3.4 x 10 4 and Ka2 = 6.7 x 10-9. What is the pH of a 0.28 M solution…

A: Given: The molarity of the solution of H2A is 0.28 M The value of Ka1 is 3.4 x 10-4 The value of Ka2…

Q: What is the pH of a 1.25 M solution of HCIO? HCIO (aq) + H20 (1) = H3O* (aq) + CIO (aq) Ka =2.88 x…

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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.