The solubility of KCLO3 (s) in water increases as the.....

Explanation:

Fats

The gallbladder stores bile ( made in the liver)  which is secreted into the digestive tract to aid in the digestion of dietary fats.

Answer :Option A) The lattice energy increases as cations get smaller, as shown by LiF and KF.

Explanation : It is observed that lattice energy is mostly influenced by two main factors of an ionic solid which are;

i) The charge on the ions - As the charge of the ions increases, the lattice energy is observed to increase too.

and

ii) The radius, or size, of the ions- As the size of the ions increases, the lattice energy decreases with it.

So, here in this question the second reason is clearly observed. Hence, it is self-explained that the size of the cations are decreased in the ionic solids the lattice energy increases.

The enthalpy change (ΔH) for the neutralization of 0.1 moles of 1.0 M NaOH with 0.1 moles of 1.0 M HCl in a coffee-cup calorimeter is approximately 28.05 kJ/mol.

To calculate the enthalpy change (ΔH) for the neutralization of HCl by NaOH, you can use the equation:

ΔH = q / moles of limiting reactant

First, let's find the moles of the reactants. We have 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl. Since we know the volumes and concentrations, you can find the moles of each reactant using the formula:

moles = (volume in L) × (concentration in mol/L)

For NaOH:

moles of NaOH = (100.0 mL / 1000 mL/L) × 1.0 mol/L = 0.1 moles

For HCl:

moles of HCl = (100.0 mL / 1000 mL/L) × 1.0 mol/L = 0.1 moles

Now, you need to determine the limiting reactant. The balanced chemical equation for the neutralization of HCl by NaOH is:

NaOH + HCl → NaCl + H₂O

The stoichiometric ratio of NaOH to HCl is 1:1, which means they react in a 1:1 ratio. Since both reactants have 0.1 moles, neither is in excess. Therefore, the reactant that limits the reaction is the one that is present in the smaller amount, which is NaOH in this case.

Now, calculate the heat absorbed or released (q) using the equation:

q = mΔTC

Where:

m is the mass (in grams) of the solution, which we can calculate using the density of 1.0 g/cm³ and the volume (in mL).

ΔT is the change in temperature.

C is the specific heat capacity (given as 4.18 J/g°C).

For the volume of 100.0 mL, the mass is 100.0 g (since 100.0 mL = 100.0 g, given the density is 1.0 g/cm³).

ΔT = Final temperature - Initial temperature

ΔT = 31.38°C - 24.68°C = 6.70°C

Now, calculate q for the reaction:

q = 100.0 g × 6.70°C × 4.18 J/g°C = 2804.76 J

Finally, calculate the enthalpy change (ΔH) by dividing q by the moles of the limiting reactant:

ΔH = 2804.76 J / 0.1 moles = 28047.6 J/mol

Since the enthalpy change is typically expressed in kJ/mol, divide by 1000 to convert J to kJ:

ΔH = 28.05 kJ/mol

So, the enthalpy change for the neutralization of HCl by NaOH is approximately 28.05 kJ/mol.

To know more about moles:

brainly.com/question/34302357

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