Question

1. 100 ml of 0.2M H2SO4 is mixed with 300ml of 0.1M Ca(OH)2. Answer the following a. Is the mixture acidic, basic or neutral b. Calculate the molarity of the acid or base leftover c. Calculate the molarity of the salt formed d. Calculate the pH of the resultant mixture.

Answer 1

Answer:

•♥•♥•♥ NORMALITY OF ANY ACID OR BASE WILL BE EQUAL TO GRAM-EQUIVALENT DESOLVE IN GIVEN VOLUME ♥•♥•♥•

N = gram-equivalent/ volume(lt.)

When two or more compounds or elements react together their

gram-equivalent will be equal in simple way, 10 gm-eq of an acid will react completely with 10 gm-eq of base,

In given problem,

gm-eq. of H2SO4 = N*V(lt.)

and N = n*M where, M = molarity and n = basicity or acidity of an acid or base.

gm-eq of H2SO4 = 100*2*0.2*0.001

=0.04gm-eq

gm-eq of NaOH = 100*0.2*1*0.001

=0.02

remaining gm-eq of H2SO4 = 0.04–0.02

0.02gm-eq

Now,

gm-eq. = N*V = 0.02

Total volume =200ml = 0.2 lt.

N*0.2 = 0.02 = 0.1N

Hope you find it helpful!!!

100 mL of 0.2 M sulphuric acid (not sure how to write chemical formulae in this maths format…please comment if you know) is 20 mmol (millimoles) of sulphuric acid.

100 mL of 0.2 M sodium hydroxide is also 20 mmol.

We know that 1 mole of sulphuric acid reacts with 2 moles of sodium hydroxide.

H2SO4 + 2NaOH → Na2SO4 + 2H2O

So, in this case, we have 20 mmol NaOH reacting with 10 mmol of sulphuric acid.

So, 10 mmol sulphuric acid is left.

We know that valency factor of sulphuric acid is 2. So, 10 mmol of sulphuric acid is 20 meq (milliequivalents), in a total of 200 mL of solution.

So, the answer is (20meq)/(200mL)=0.1N

Answer 2

Answer:

1.Start with the balanced equation:

H2SO4 + 2 NaOH →. Na2SO4 + 2 H2O

Observe that 2 moles of NaOH are required to neutralize one (1) mole of H2SO4.

So what do we have to work with?

O.100 L H2SO4 x 0.2 moles/ L = 0.02 moles H2SO4

0.100 L NaOH x 0.2 moles/ L = 0.02 moles NaOH

Therefore the 0.02 moles of NaOH will neutralize 0.01 moles H2SO4.

This leaves 0.01 moles of H2SO4 in 0.2 L of solution.

We want to know the Normality of the solution after the reaction.

0.01 moles H2SO4 /0.200 L = x moles / one (1) L. x = 0.05 moles / L

Since H2SO4 is dibasic there are 2 equivalents per mole. Therefore the solution has 0.05 x 2 = 0.1 equivalents per L which is 0.1 Normal.

2a.Is acidic basic or neutral?

The pH scale ranges from 0 to 14. A pH of 7 is neutral. A pH less than 7 is acidic. A pH greater than 7 is basic.