9. Which acid has the strongest conjugate base? A. H2O2 B. H2CO3 C. HCO3- D. HC2O4- 10. How many hydroxide ions are there in one litre of water? A. none C. approximately 1 x 10-14 mol B. approximately 1 x 10-7 mol D. Approximately 1 x 100 mol 11. Determine the products of the reaction between the following reactants. HSO3- + H2PO4- à ? + ? A. SO32- + H3PO4 C. H2SO3 + HPO42- B. water and a salt D. H3O+ and OH- only 12. True or false: A basic solution will turn only to yellow when tested with methyl orange indicator. A. True B. False
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.
Just solve question 9-12, thanks.
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1. |
What is the value of Kb for H2PO4-? A. 1.3 x 10-12 B. 1.6 x 10-7 C. 6.2 x 10-8 D. 7.5 x 10-3 |
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2. |
Which of the equations has a Bronsted-Lowry conjugate acid-base pair? A. 2H2 + O2 ß à H2O C. Zn + 2HCl à H2 + ZnCl2 B. NaOH à Na+ + OH- D. H2O + HCN ßà H3O+ + CN- |
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3. |
What is the conjugate base of HSO4-(aq)? A. OH-(aq) B. H2SO4(aq) C. H3O + (aq) D. SO4 2-(aq) |
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4. |
Which term describes a substance that acts as a proton donor and a proton acceptor? A. amphoteric B. monoprotic C. polyprotic D. acid-base |
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5. |
What is t What is the concentration of hydroxide ions in a solution of 0.350 mol/L HCl(aq)? A. 0.350 mol/L B. 0.175 mol/L C. 2.86 x 10-14 mol/L D. 0.650 mol/L |
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6. |
A solution contains 3.3 x10-8 M hydroxide ions. What is the pH of the solution? A. 3.25 B. 6.51 C. 7.49 D. 8.00 |
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7. |
A solution has a pH of 4.65. What is the concentration (in M) of hydroxide ions in the solution? 1.0 x 10-14 B. 4.5 x 10-10 C. 1.0 x 10-7 D. 2.2 x 10-5 |
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8. |
Which solution would have the greatest conductivity? (HINT: conductivity increases as dissociation increases)? A. 0.1M HCl B. 0.1 M HCO3- C. 0.1 M H2CO3 D. 0.1 M HC2O4 |
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9. |
Which acid has the strongest conjugate base? A. H2O2 B. H2CO3 C. HCO3- D. HC2O4- |
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10. |
How many hydroxide ions are there in one litre of water? A. none C. approximately 1 x 10-14 mol B. approximately 1 x 10-7 mol D. Approximately 1 x 100 mol |
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11. |
Determine the products of the reaction between the following reactants. HSO3- + H2PO4- à ? + ? A. SO32- + H3PO4 C. H2SO3 + HPO42- B. water and a salt D. H3O+ and OH- only |
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12. |
True or false: A basic solution will turn only to yellow when tested with methyl orange indicator. A. True B. False |
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