A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10-10.

Since Q > Ksp, a precipitate of AgCl will form.

Explanation:

Step 1: Data given

Molarity AgNO3 = 0.10 M

Molarity of NaCl = 0.075 M

Ksp AgCl = 1.77 * 10^-10

Step 2: The balanced equation

AgNO3 + NaCl → AgCl(s) + NaNO3(aq)

For 0.10 moles AgNO3 we have 0.10 moles Ag+ ( molarity = 0.10 M)

For 0.075 moles NaCl we have 0.075 moles Cl- (molarity = 0.075 M)

Step 3: Calculate Q

Q = [Ag+][Cl-]

Q = (0.10 M )(0.075 M ) = 0.0075

Ksp = 1.77 * 10^-10

Q >>> Ksp

Since Q > Ksp, a precipitate of AgCl will form.

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.