A solution is prepared by dissolving 23.8 g of ammonium sulfate in enough water to make 100.0 mL of stocksolution. A 11.50-mL sample of this stock solution is added to 51.10 mL of water. Calculate the concentration of ammonium ions andsulfate ions in the final solution.
NH4+ M SO42? M
A solution is prepared by dissolving 23.8 g of ammonium sulfate in enough water to make 100.0 mL of stocksolution. A 11.50-mL sample of this stock solution is added to 51.10 mL of water. Calculate the concentration of ammonium ions andsulfate ions in the final solution.
| NH4+ | M |
| SO42? | M |
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Principles of Chemistry Molecular Approach
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
Chemistry: The Central Science
Related questions
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane.
2 NH3(g) + 3 O2(g) + 2 CH4(g) â 2 HCN(g) + 6 H2O(g)
If 5.29 â 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
| HCN | g |
| H2O | g |
A solution is prepared by dissolving 14.4 g ammonium sulfate in enough water to make 113.0 mL of stock solution. A 13.20-mL sample of this stock solution is added to 52.30 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
An 11.7-L sample of gas is determined to contain 0.40 mol N2. At the same temperature and pressure, how many moles of gas would there be in a 10.-L sample?
