2. Calculate the number of grams of potassium iodide (KI), needed to prepare 500.0 mL of a 0.125 M KI. Show your work.

For the preparation of 0.125 M of KI solution, 10.37 grams of KI is needed.

Molarity can be defined as the moles of solute in a liter of solution.

Molarity =

Given, Molarity = 0.125 M

volume = 500 ml

We know the molecular weight of KI = 166.002 g/mol

Putting the values in the equation:

0.125 M =

weight =

weight of KI = 10.37 grams.

For the preparation of 0.125 M of KI solution, 10.37 grams of KI is needed.

For more information about molarity, refer to the link:

link

10.38 g

Explanation:

From the question given above, the following data were obtained:

Volume of solution = 500 mL

Molarity of KI solution = 0.125 M

Mass of KI needed =?

Next, we shall convert 500 mL to litres (L). This can be obtained as follow:

1000 mL = 1 L

Therefore,

500 mL = 500 mL × 1 L / 1000 mL

500 mL = 0.5 L

Thus, 500 mL is equivalent to 0.5 L.

Next, we shall determine the number of mole KI in the solution. This can be obtained as illustrated below:

Volume of solution = 0.5 L

Molarity of KI solution = 0.125 M

Mole of KI =?

Molarity = mole /Volume

0.125 = mole of KI /0.5

Cross multiply

Mole of KI = 0.125 × 0.5

Mole of KI = 0.0625 mole

Finall, we shall determine the mass of KI needed to prepare the solution as follow:

Mole of KI = 0.0625 mole

Molar mass of KI = 39 + 127 = 166 g/mol

Mass of KI =?

Mole = mass /Molar mass

0.0625 = mass of KI /166

Cross multiply

Mass of KI = 0.0625 × 166

Mass of KI = 10.38 g

Therefore, 10.38 g is needed to prepare the solution.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

answer:

technetium is the most reactive. this is followed by silver. the least reactive out of these three elements is strontium.