Which reaction would produce a solution that conducts electricity extremely well? h3po3(aq) mc032-1.jpg h+(aq) + h2po3–(aq) ch3ch2cooh(aq) + h2o(l) mc032-2.jpg h3o+(aq) + ch3ch2coo–(aq) ch3ch2oh(l) mc032-3.jpg ch3ch2oh(aq) ca(no3)2(s) mc032-4.jpg ca2+(aq) + 2no3–(aq)

The correct answer is

Explanation:

A strong electrolyte is defined as the electrolyte which completely dissociates into its ions when dissolved in water.

A weak electrolyte is defined as the electrolyte which does not completely dissociates into its ions when dissolved in water.

A solution having more number of ions will easily conduct electricity.

For the given chemical equations:

1.

It is a weak electrolyte because it is not completely dissociated and number of ions present are 2.

2.

It is a weak electrolyte because it is not completely dissociated and number of ions present are 2.

3.

Here, hydration of ethanol is taking place and no ions are present in the solution.

4.

It is a strong electrolyte because it is has completely dissociated into its ions and number of ions present are 3 and thus it will conduct electricity.

Therefore, the solution which will conduct electricity extremely well will be

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