g A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 22.69 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is

The question is incomplete, the complete question is:

A solution of permanganate is standardized by titration with oxalic acid. To react completely with 0.0018 mol of oxalic acid required 22.69 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:

Determine the concentration of the permanganate solution in molarity.

The molarity of permanganate solution is 0.0317 M

Explanation:

The balanced chemical equation follows:

Given values:

Moles of oxalic acid = 0.0018 moles  

By the stoichiometry of the reaction:

If 5 moles of oxalic acid reacts with 2 moles of permanganate solution

So, 0.0018 moles of oxalic acid will react with = of permanganate solution

The formula used to calculate molarity:

.....(1)

Given values:

Moles of permanganate solution = 0.00072 moles

Volume of solution = 22.69 mL

Putting values in equation 1, we get:

Hence, the molarity of permanganate solution is 0.0317 M

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol