calculate the amount of solid NH4Cl to add to 50 mL of 1 M ammonia to form a mixture that has a pH of 9 assume no volume change in the solution

I told you what to use at your original post. What's the problem?

i did it before you answered it i just wanteed to rewrite it out correctly

To calculate the amount of solid NH4Cl to add to 50 mL of 1 M ammonia to form a mixture with a pH of 9, we need to consider the acid-base reaction between ammonia (NH3) and ammonium chloride (NH4Cl).

First, let's write the balanced chemical equation for the reaction:

NH3 + H2O ⇌ NH4+ + OH-

In this reaction, ammonia acts as a weak base, and water acts as an acid, forming ammonium (NH4+) and hydroxide (OH-) ions.

We know that the pH of a solution is related to the concentration of hydroxide ions (OH-). The higher the concentration of OH-, the more basic (higher pH) the solution will be.

To achieve a pH of 9, we need to calculate the concentration of OH- ions in the final solution and then use that to determine the amount of ammonium chloride needed.

From the balanced equation, we see that one molecule of ammonia (NH3) reacts with one molecule of water (H2O) to form one ammonium ion (NH4+) and one hydroxide ion (OH-).

Therefore, the concentration of OH- ions will be equal to the concentration of ammonia (NH3) that reacts in the reaction.

Since we have 50 mL of 1 M ammonia, we have 0.05 moles of ammonia (1 M * 0.05 L = 0.05 moles NH3).

According to the stoichiometry of the balanced equation, this means we will have 0.05 moles of NH4+ and 0.05 moles of OH- ions.

Now, let's calculate the volume of the final solution. Since there is no volume change, it will remain at 50 mL or 0.05 L.

To find the concentration of OH- ions, we divide the moles by the volume in liters:
0.05 moles OH- / 0.05 L = 1 M OH- concentration.

Since the concentration of OH- ions is equal to the ammonia concentration, we need to neutralize this concentration by adding enough ammonium chloride (NH4Cl) to react with all the OH- ions.

From the balanced equation, we see that one hydroxide ion (OH-) reacts with one ammonium ion (NH4+).

So, to neutralize 1 M of OH- ions, we need to add 1 M of ammonium chloride (NH4Cl).

Therefore, to achieve a pH of 9, you need to add 1 M of solid NH4Cl to the 50 mL of 1 M ammonia solution.

Please note that this calculation assumes ideal behavior and that there are no other factors that might affect the pH, such as the formation of additional ions or complexation reactions.