1.Which acid is strongest? a. H3AsO3, Ka=5.1x10-10 b. HCN, Ka=4.9x10-10 c. H3BO3, Ka=5.8x10-10 d. C6H5OH, Ka=1.3x10-10 2. If [H+] in a solution at SATP is 6.3x10-6M, [OH-]= a. 5.2 M b. 5.3x10-8M c. 1.6x10-9M d. 3.7x10-8M 3.If the pOH of a solution is 7.0, the pH is
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.
1.Which acid is strongest?
| a. | H3AsO3, Ka=5.1x10-10 |
| b. | HCN, Ka=4.9x10-10 |
| c. | H3BO3, Ka=5.8x10-10 |
| d. | C6H5OH, Ka=1.3x10-10 |
2. If [H+] in a solution at SATP is 6.3x10-6M, [OH-]=
| a. | 5.2 M |
| b. | 5.3x10-8M |
| c. | 1.6x10-9M |
| d. | 3.7x10-8M |
3.If the pOH of a solution is 7.0, the pH is
| -7.0 | |
| 1.0x10-7 | |
| 0.14 | |
| 7.0 |
4.Which of the following is not an
| HI(aq) | |
| CH3COOH(aq) | |
| KOH(aq) | |
| NH4+(aq) |
5.Doubling the pH means changing the hydrogen ion concentration by
| a factor of 2x | |
| a factor of 20x | |
| a small fraction of a the original | |
| up to 107x |
6.Which solution has the highest pH?
| 3.9x10-3 M HPO42- (Ka3=4.2x10-13) | |
| 2.1x10-6M HONH2 (Kb=1.1x10-8) | |
| 0.00072 M C6H5NH2 (Kb=4.3x10-10) | |
|
1.1x10-7M LiOH |
7.A weak acid
| doesn't react very much | |
| can't react as well with strong bases | |
| tends to remain in molecular form | |
| has a much higher pH |
8.In the equilibrium, F-(aq)+HO2CCO2H(aq)⇄HF(aq)+HO2CCOO-(aq), HF is the
| acid | |
| base | |
| conjugate acid | |
| conjugate base |
10.Which of these solutions could have a pH of 5.0?
| H2SO4 | |
| LiOH | |
| Mg(OH)2 | |
| CH3NH2 |
11.The pH of a 0.0200 M LiOH solution is
| 1.7 | |
| 3.9 | |
| 10.1 | |
| 12.3 |
12.Kb for 0.100 M phenol, whose pH is 8.82 is
| 2.3x10-17 | |
| 1.5x10-9 | |
| 4.4x10-10 | |
| 1.5x10-4 |
13.
| 2.8 | |
| 0.13 | |
| 1.3 | |
| 0.90 |
Which of the following is a Brønsted-Lowry acid-base reaction?
| CO32-(aq)+CH3COOH(aq)⇄HCO3-(aq)+CH3COO-(aq) | |
| K(s)+2H2O(l)⇄KOH(aq)+H2(g) | |
| NH3(g)+HCl(g)→NH4Cl(s) | |
| 2HCOOH(aq)+O2(aq)⇄2CO2(aq)+2H2O(l) |
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