Question

question 1 (1 point)
Saved
A 15.0 ml sample of LiOH solution reaches equivalence point when 25.0 ml of 0.10M HCl is added. The original [LiOH] is

Question 1 options:

0.60 M


0.060M


0.17 M


0.0025M

Question 2 (1 point)
Saved
Naturally occuring, unpolluted rain water is slightly acidic. Why is this?

Question 2 options:

Due to the presence of dissolved nitrogen dioxide.


Due to the presence of dissolved methane.


Due to the presence of dissolved carbon dioxide.


Due to the presence of dissolved oxygen.

Question 3 (1 point)
Saved
Which of the following indicators would be best when titrating NH3(aq) with HBr(aq)?

Question 3 options:

Alizarian yellow


Phenolphtalein


Methyl violet


Methyl orange

Question 4 (1 point)
Saved
How many moles of Ca(OH)2 are required to neutralize 20.00 mL of 0.100 M HCl ?

Question 4 options:

1.0 x 10-3 moles


4.0 x 10-3 moles


2.0 x 10-3 moles


0.10 moles

Question 5 (1 point)
Saved
With which of the following will water act as an acid?

Question 5 options:

NH3


H3O+


HClO4


NH4+

Question 6 (1 point)
Saved
What is the value of Kb for the conjugate base of H3BO3?

Question 6 options:

6.5 x 104


1.5 x 10-5


1.5 x 109


6.5 x 10-10

Question 7 (1 point)
Saved
Which of the following solutions would have a pH less than 7?

Question 7 options:

aluminum (III) chloride


sodium acetate


lithium chloride


potassium sulphide

Question 8 (1 point)
Saved
Which of the following would produce the most acidic solution?

Question 8 options:

NaClO4


NH3


H2O2


H2O

Question 9 (1 point)
Which ionic compound will create an acidic solution when dissolved?

Question 9 options:

KCN


NaCl


NH4I


NaHS

Question 10 (1 point)
Saved
Which of the following acids is the strongest?

Question 10 options:

HCN


H2S


CH3COOH


HNO2

Question 11 (1 point)
Two unknown solutions contain 1.0 M HCl for the first and the second contains water. To distinguish between the two solutions, one would use

Question 11 options:

none of these will distinguish between the two solutions


red litmus


phenolphthalein


magnesium

Question 12 (1 point)
Sodium potassium tartrate (NaKC4H4O6) is used to raise the pH of fruit during processing. In this
process, sodium potassium tartrate is being used as a/an

Question 12 options:

acid


buffer


salt


base

Question 13 (1 point)
What is the [OH- ] in a solution where [H3O+ ] = 2.0 M at 25 degrees C?

Question 13 options:

5.0 x 10-15M


12 M


5.0 x 10-13 M


2.0 x 10-14 M

Question 14 (1 point)
Which of the following substances is/are amphiprotic?

I. H2A

II. HA-

III. A2-

Question 14 options:

II only


I only


I and II


II and III

Question 15 (1 point)
The pH of an acid is 3.32. The [OH-] would be

Question 15 options:

2.1 x 10-11


4.8 x 10-4


1.0 x 10-7


1.0 x 10-14

Question 16 (1 point)
Which of the following compounds would produce an acidic solution when dissolved in water?

Question 16 options:

MgO


K2O


FeO


CO2

Question 17 (1 point)
Which of the 2 substances in the equilibrium below are Bronstead-Lowry bases?

HA- + B2- ↔ HB- + A2-

Question 17 options:

A2- and B2-


HB- and A2-


B2- and HB-


HA- and HB-

Question 18 (1 point)
A solution of RbNO2 will be

Question 18 options:

neutral


basic


acidic


can not be determined

Question 19 (1 point)
Which of the following will form a buffer system?

Question 19 options:

SO42- and SO32-


NH3 and NH2-


H2SO4 and HSO4-


H2CO3 and HCO3-

Question 20 (1 point)
The pH of a 0.10M solution of NaHSO3 is approximately

Question 20 options:

1


4


7


10