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Acids and Bases: Identifying Acidic and Basic Salts

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Wize University Chemistry Textbook > Acids and Bases

Salts

6 Activities

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Mark Yourself Question
  1. Grab a piece of paper and try this problem yourself.
  2. When you're done, check the "I have answered this question" box below.
  3. View the solution and report whether you got it right or wrong.
Consider four different aqueous salt solutions, each of which has an initial concentration of 0.100 M and undergoes complete dissociation to its ions. For each solution (each row),
  1. Identify any ions produced which act as acids or bases.Omit any ion that does not act as either an acid or base. You may leave boxes empty if no ions meet that description.
  2. Classify the solution pH as overall acidic, basic or neutral:
Ions in this solutionwhich act as acidsIons in this solutionwhich act as basesSolution pH (choose from acidic, basic or neutral)NaN3CaCO3BaI2\def\arraystretch{3} \begin{array}{c:c:c:c} \hline &\rm Ions\ in\ this\ solution \atop \rm which\ act\ as \ acids &\rm Ions\ in\ this\ solution \atop \rm which\ act\ as \ bases & \rm Solution\ pH\ \atop \rm (choose \ from \ \bold{acidic, \ basic \ or \ neutral})\\ \hline NaN_3 & & & \\ \hline CaCO_3& & & \\ \hline BaI_2\\ \hline \end{array}
More Salts Questions:
If a strong base is mixed with an equally but oppositely strong acid, what is the relative pH of the resulting salt?
Explain whether an aqueous solution of each of these salts is acidic, basic or neutral:
KBr,
NH4Cl,
Explain whether an aqueous solution of each of these salts is acidic, basic or neutral:
KBr,
NH4Cl,
Acids and Bases: pH of Salt Solutions
If each of the following salts are dissolved in water, determine if the pH will be >7, <7 or =7.
a) KBr
b) Na3PO4
Salts
Determine whether the following salts, when dissolved in water, will have a pOH > 7, pOH < 7 or a pOH = 7 (Enter your answers as: >7, <7 or =7
Strength of Acids and Bases
Will the following salts, when dissolved in water, result in an acidic, basic or neutral solution?
Strength of Acids and Bases
Will the following salts, when dissolved in water, result in an acidic, basic or neutral solution?
Which one of the following salts will form a neutral solution on dissolving in water?
A series of solutions are formed with strontium salts of the form SrX2 where X=F, Cl, Br, I.
Which of the solutions will have the highest pH?
Pure water has a pH of 7.00. 1.1g of MgBr2 is added to 15L of pure water. The solubility of MgBr2 in water is approximatly 101.5g/L. What is the pH of the resulting solution?
Acids and Bases: Salt
Is an aqueous solution of each of these salts acidic, basic or neutral?
Which one of the following salts will form a neutral solution on dissolving in water?
Practice: Salts of acids and bases
Consider four different aqueous salt solutions, each of which has an initial concentration of 0.100 M and undergoes complete dissociation to its ions. For each solution (each row),
identify any ions produced which act as acids or bases. If no ions meet that description, enter "DNE" (does not exist) inside the box
classify the solution pH as overall acidic, basic or neutral: