17. Acid and Base Equilibrium

Ionic Salts

17. Acid and Base Equilibrium

Ionic Salts

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Ionic Salts - Cations

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How to Determine if Salt is Acidic, Basic, or Neutral Example, Problem, Shortcut, Explained Question

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Acidic, Basic, and Neutral Salts - Ionic Compounds

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Acid–base properties of salts | Acids and bases | AP Chemistry | Khan Academy

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pH of salt solutions | Acids and bases | Chemistry | Khan Academy

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16.5 Acidity and Basicity of Salts

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Practice this topic

Multiple Choice

Determine if each of the following compounds will create an acidic, basic or neutral solution.

a) LiC₂H₃O₂b) C₆H₅NH₃Br

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Multiple Choice

Determine if each of the following compounds will create an acidic, basic or neutral solution.

a) Co(HSO₄)₂ b) Sr(HSO₃)₂

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Multiple Choice

Determine if each of the following compounds will create an acidic, basic or neutral solution.

a. C₃H₇NH₃F

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Multiple Choice

Determine the pH of a 0.55 M NaCN solution. The Ka of hydrocyanic acid, HCN, is 4.9 x 10^-10.

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Multiple Choice

Which of the following compounds would decrease the pH of solution?

a) SrBr₂ b) KSH c) NaN₃ d) NiP e) Hg₂Cl₂

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Multiple Choice

Which of the following compounds would increase the pH of solution?

a) SrBr₂ b) K c) NaN₃ d) NiBr₂ e) Hg₂Cl₂

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Multiple Choice

Which of the following compounds would have an increase in solubility when placed into an acidic solution?

a) CaBr₂ b) NaI c) KCN d) LiNO₃ e) Hg₂Br₂

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Textbook Question

(b) If a limestone sculp- ture were treated to form a surface layer of calcium sul- fate, would this help to slow down the effects of acid rain? Explain.

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Textbook Question

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (c) NaClO4

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Textbook Question

Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (c) Na2CO3

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (e) Na2SO3.

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (c) NaClO

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (b) NaBr

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AlCl3

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (d) 3CH3NH34NO3

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Textbook Question

An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08. What is the identity of the salt?

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Textbook Question

An unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 0.100 M solution of the salt is neutral, what is the identity of the salt?

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Textbook Question

Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3-

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Textbook Question

Indicate whether each of the following statements is correct or incorrect. (d) K+ ion is acidic in water because it causes hydrating water molecules to become more acidic.

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Textbook Question

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+

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Textbook Question

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+

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Textbook Question

Determine if each compound is more soluble in acidic solution than it is in pure water. Explain. c. AgCl

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Textbook Question

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+

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Textbook Question

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+

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Textbook Question

Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li+

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Textbook Question

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO2

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Textbook Question

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3

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Textbook Question

Arrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH

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Textbook Question

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) AgBr

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Textbook Question

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (b) Fe(OH)3

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Textbook Question

Write a balanced net ionic equation for the principal reaction in solutions of each of the following salts. In each case, identify the Brønsted–Lowry acids and bases and the conjugate acid–base pairs. (a) Na2CO3

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Textbook Question

Classify each of the following ions according to whether they react with water to give a neutral, acidic, or basic solution. (a) F-

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Textbook Question

Classify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for values of equilibrium constants. (a) Fe1NO323

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Textbook Question

Calculate Ka for the cation and Kb for the anion in an aqueous NH4CN solution. Is the solution acidic, basic, or neutral?

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Textbook Question

The hydrated cation M1H2O26 3 + has Ka = 10-4, and the acid HA has Ka = 10-5. Identify the principal reaction in an aqueous solution of each of the following salts, and classify each solution as acidic, basic, or neutral. (a) NaA

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Open Question

Classify each of the following anions as basic or neutral.

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Open Question

Arrange the following solutions in order of increasing acidity:

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