16) Which acid is stronger between the acids noted in two previous problems? The
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16) Which acid is stronger between the acids noted in two previous problems? The Ka of H3PO4 is 7.1x 103 while for ILs it is 7.1x 17) Which of these is a strong acid. H2So or HF? 18) How do buffers differ from other acids and bases? 19) When a base is added to a buffer, what does the buffer do to prevent pH change? 20 When an acid is added to a buffer, what does the buffer do to prevent pH change? 21) which of these compounds is capable of forming a bufer, Heso and Has? The K. of H2so is 1.1x 103 while for H2S it is 7.1x 10 22) Describe the term activation energy and provide an example for a chemical reaction or physical process not covered in class (Nothing allowed on boulders nor matches). 23) Which of these characteristics ofreactions do catalysts affect: whether reaction is spontaneous or not, the equilibrium of reaction, and/or the speed of a reaction? 24 You have a nitric acid solution of unknown concentration. In the lab you find that titration of 17.01 mL of HNOs requires 26.23 mL of 1.000 M NaoH. What is the molarity of this HNO, solution? 25)In this problem the concentration of the nitric acid solution is known. What volume of 0.400 M NaoH will be required to titrate 25.00 mL of a 0.200 M HNOs solution?Explanation / Answer
16) H3PO4 with higher Ka is stronger acid than H2S
17) H2SO4 is a strong acid
18) Buffer have both acid and base component present in solution
19) When base is added, it reacts with acid component of buffer and resist changes in pH
20) When acid is added, it reacts with base component of buffer and resist changes in pH
21) H2S a weak acid can form buffer solution
22) Activation energy is energy needed for reactants to have before it forms the products. Say for the formation of tert-butyl alcohol from tert-butylchloride would need activation energy to form carbocation in the first step.
23) Characteristic of reaction affected by catalyst : speed of reaction
24) moles of HNO3 = moles of NaOH = 1 M x 26.23 ml = 26.23 mmol
molarity of HNO3 = 26.23 mmol/17.01 ml = 1.542 M
25) moles of NaOH = moles of HNO3 = 0.2 M x 25 ml = 5 mmol
Volume of NaOH needed = 5 mmol/0.4 M = 12.5 ml
1) pH = -log[H3O+] = 8.2
[H3O+] = 6.31 x 10^-9 M
2) [H3O+] = 2.1 x 10^-6 M
pH = -log(2.1 x 10^-6) = 5.68
3) pH = -log[H3O+] = 7.4
[H3O+] = 3.98 x 10^-8 M
4) [H3O+] = 1 x 10^-14/[OH-] = 1 x 10^-14/4.3 x 10^-7 =
pH = -log[H3O+] = 7.63
5) [H3O+] = 1 x 10^-14/[OH-] = 1 x 10^-14/7.6 x 10^-1 =
pH = -log[H3O+] = 13.88
6) [H3O+] = 1 x 10^-4 M when pH = 4
[H3O+] = 1 x 10^-7 when pH = 7
ratio (pH 4/pH 7) = 1000
7) [H3O+] = 1 x 10^-8 M when pH = 8
[H3O+] = 1 x 10^-10 when pH = 10
ratio (pH 4/pH 7) = 100
8) According to bronsted-Lowry acid-base concept, acid is one which donates an H+ and base is one that accepts H+ ion to form conjugate acid of base.
9) Amphiprotic is a species that may either donate an H+ and act as an acid or may accept a H+ and act as a base in solution.
10) HCO3- is amphiprotic
11) NH4+ is an acid
12) CO3^2- is a base
13) conjugate base of HNO3 is NO3-
14) conjugate base of H2S is HS-
15) conjugate base of H3PO4 is H2PO4-
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