Question

For reactions 1 and 2, calculate the moles of NH4Cl produced or dissolved. Given: Volume HCl...

For reactions 1 and 2, calculate the moles of NH4Cl produced or dissolved.

Given:

Volume HCl (50.0mL), Mass HCl (51.5g), Volume NH3 (50.0mL), Mass of NH3 (51.5g), Molarity of HCl (0.9847), molarity of NH3aq (1.1mol/L).

In Reaction 1, calculate the moles of NH4Cl by using molarity (M) and volume (L) of the limiting reagent, HCl.

In Reaction 2, this can be found from the mass of the NH4Cl used and it's molar mass (53.49g/mol)

Please show step by step. Thank you. :)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The total number of moles (n) of a solute is equal to the given mass of the solute divided by molar mass of the solute. The molarity (M) is defined as the total number of moles of solute per litre volume of the solution. The detailed solution is given below:

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the molar mass of NaHCO3(s), Na2CO3(s), and CO2(g) Calculate the number of moles of HCl...
Calculate the molar mass of NaHCO3(s), Na2CO3(s), and CO2(g) Calculate the number of moles of HCl contained in the two volumes of HCl solution (25.0ml and 50.0mL: remember to use the molarity of the solution rather than the molar mass of HCl to find molarity).
1. NH4Cl(aq)<->NH3(g) + HCl(aq) Using the standard thermodynamic data in the tables linked above, calculate the...
1. NH4Cl(aq)<->NH3(g) + HCl(aq) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. 2. HCl(g) + NH3(g)NH4Cl(s) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.
1.)What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and...
1.)What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25mL of 12 M NH3 in enough water to make 1.00L of solution? Kb=1.80x10-5 for NH3. Calculate the change in pH after addition of 50.0mL of 0.15M NaOH. 2.)What mass of Na2SO4 (molar mass=142.0 g/mol) must be added to 350mL of 0.16M Ag+ to initiate precipitation of Ag2SO4? The Ksp of Ag2SO4 is 1.2x10-5. Assume no volume change occurs upon addition of Na2SO4. 3.)What...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate The mass of sodium chloride in (g) is...
Nitronium cation formation:: 1. Show the steps to calculate theoretical yield of nitronium ion (NO2+) in...
Nitronium cation formation:: 1. Show the steps to calculate theoretical yield of nitronium ion (NO2+) in moles? Molecular weight of NO2+ is 46.01 g/mol. HNO3: molarity = 15.8 mol/L molecular weight = 63.01 g/mol volume added = 1 mL moles added = 0.0158 mol H2SO4: molarity = 18.4 mol/L molecular weight = 98.08 g/mol volume added = 2 mL moles added = 0.0372 mol Nitration of Methyl Benzoate:: 2. Calculate volume added (mL) of NO2+ AND moles (mol) added of...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate The mass of sodium chloride in (g) is...
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL)...
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL) = 25.0 mL 2. Concentration of Standardized HCL solution (mol/L) = 0.05 mol/L 3. Buret reading, initial (mL) = 50.0 mL 4. Buret reading, final (mL) = 32.5 mL 5. Volume of HCL added (mL) = 17.5 mL 6. Moles of HCL added (mol) = (concentration of HCl)(Volume of HCl) = (0.05)(19.1) = 0.875 mol. 7.Moles of OH- in saturated solution (mol)=8.75x10^-4 8.the [OH-]...
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +     
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +        6H2O(l) How many moles of water are produced when 4.5 moles of oxygen react?        (Hint: Use slides 5-8) 2. Given: I2     +    3 F2      ®     2 IF3 How many moles of I2 are needed to form 3 moles of IF3? How many moles of F2 are needed to form 10 moles of IF3? How many moles of I2 are needed to react with 3.5 moles of F2?        ...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M...
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate The mass of sodium chloride in (g) is...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl...
For the next three problems, consider 1.0 L of a solution which is 0.3 M NH4Cl and 0.2 M NH3 (Ka for NH4Cl = 5.6 x 10-10). Assume 2 significant figures in all of the given concentrations so that you should calculate all of the following pH values to two decimal places. 1. Calculate the pH of this solution. 2. Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT