Answer:
Answer : (1) :-
Volume of water filled in the pycnometer is given as = 9.9872 mL.
Mass of pycnometer when filled with water = 23.1148 g.
Mass of empty pycnometer = 13.1455 g.
So, mass of water = (23.1148 - 13.1455) g. = 9.9693 g.
We know that,
<em> Density = Mass / Volume = (9.9693 g.) / (9.9872 mL) = </em>0.998 g/mL.
<u>It is observed that the density of water is evaluated to be 0.998 g/mL. We know that, at 4℃ the density of water becomes maximum i.e. 1 g/mL. On the other hand the temperature at which the density of water is 0.998 g/mL is 0℃. Therefore, it can be concluded that the experiment was performed at a temperature of 0℃.</u>
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1.5M NaOH so we've 1.5 moles of NaOH in 1L of solution
1L = 1000 ml
1.5 moles of NaOH ------------in------------- 1000 ml
0.75 moles of NaOH ----------in---------------x ml
x = 500 ml
<em><u>answer: C</u></em>
I think this is what you wanted, so good luck!
Answer: 16.32 g of 
as excess reagent are left.
Explanation:
To calculate the moles :
According to stoichiometry :
2 moles of 
require = 1 mole of
Thus 0.34 moles of will require=
of
Thus is the limiting reagent as it limits the formation of product and is the excess reagent.
Moles of left = (0.68-0.17) mol = 0.51 mol
Mass of 
Thus 16.32 g of as excess reagent are left.
