It is the point when enough analyte has been added.
It is the point when the amount of added titrant is equal to the amount of analyte in the solution.
It is the point when the volume of titrant is equivalent the volume of analyte.
It is the point when the concentration of titrant added is equivalent to the volume of analyte.
Q.2.
What is the role of an indicator in a reaction?
To help reactants react successfully.
To bind to the analyte to form a products.
To show when the reaction has reached or past the equivalence point.
To provide a surface for the reaction to occur.
Q.3.
How will I ensure I get an accurate final end point?
Be slow and careful
Repeat until you have 3 very similar titre
Rinse the Burette
Always use the same Pipette filler
Q.4.
What term describes the change in color of the indicator during a titration?
colorizing
endpoint
equivalence point
endgame
Q.5.
A student used a 0.M of sodium hydroxide solution in a titration experiment. The initial reading on the buret was 0.mL. After the titration, the buret reading was 14.mL. How many moles of sodium hydroxide was used?
1.82 moles
1.82 x 10-3 moles
8.34 x 10-3 moles
8.6 moles
Q.6.
HCl + NaOH →
NaH + ClOH
NaCl + H2
NaCl + H2O
NaCl + Cl2
Q.7.
Acid + Base ₋-->
salt + hydrogen
salt + water
salt + carbon dioxide + water
salt
Q.8.
In which of the following reactions does H2POact as an acid?
H3PO4 + H2O --> H3O+ + H2PO4-
H2PO4- + H2O --> H3O+ + HPO42-
H2PO4- + OH- --> H3PO4 + O2-
The ion cannot act as an acid
Q.9.
I have 25mL ofHCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
0.8 M
1 M
1.25 M
Q.10.
What is the initial pH value when ethanoic acid was added into sodium hydroxide?
13.0
11.0
3.5
2.0
Q.11.
The pH at the equivalence point of the titration of a weak acid with a strong base is usually:
acidic 3.9
acidic 4.5
neutral 7.0
basic 8.2
Q.12.
What is mean by equivalence point
a point which complete neutralisation occur where indicator change colour
a point which complete neutralisation occur where volume of H+ is equal to volume of OH-
a point where pH is equal to pKa
Q.13.
Which of the following indicator is suitable for weak acid weak base titration
phenolphthalein
methyl orange
litmus
none above is suitable
Q.14.
Identify the strongest acid
HCN
H2O
CH3OH
HNO3
Q.15.
What is the endpoint of a titration
Where the amount of acid and base are equal as shown by a colour change
Where there is no base
When the volume of base in the burette is used up
When there is no acid
Q.16.
Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion in solution in largest concentration, other than the K+ ion, is
H2PO4 –
HPO4 2–
PO4 3–
OH-
Q.17.
In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment?
The [H+] at the equivalence point equals the ionization constant of the acid.
The pH at the equivalence point depends on the indicator used.
The graph of pH versus volume of base added rises gradually at first and then much more rapidly.
The graph of pH versus volume of base added shows no sharp rise.
Q.18.
Ascorbic acid, H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10–5 and K2 = 1.6 × 10–In a 0.M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration?
H3O+(aq)
H2C6H6O6(aq)
HC6H6O6-(aq)
C6H6O62-(aq)
Q.19.
How many mL of a 0.M NaOH solution are needed to neutralizemL of 0.M H3PO4 solution?3NaOH (aq) + H3PO4 (aq) ----> Na3PO4 (aq) + 3H(l)
7.5 mL
0.015 mL
68 mL
23 mL
Q.20.
What is the main purpose of acid-base titrations?
To test if reactants react.
To calculate the concentration of unknown analyte.
To calculate the concentration of known analyte.
To test quality of reactants.
Support mcqgeeks.com by disabling your adblocker.
Please disable the adBlock and continue. Thank you.