Westonci.ca is the premier destination for reliable answers to your questions, provided by a community of experts. Connect with a community of experts ready to help you find solutions to your questions quickly and accurately. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.
Sagot :
To determine the number of moles of ions formed when 65.25 g of barium nitrate (Ba(NO₃)₂) dissolves in water, follow these steps:
### Step 1: Calculate the molar mass of barium nitrate (Ba(NO₃)₂)
To find the molar mass, sum up the atomic masses of all the atoms in the formula.
1. Atomic mass of Barium (Ba): 137 g/mol
2. Atomic mass of Nitrogen (N): 14 g/mol
3. Atomic mass of Oxygen (O): 16 g/mol
4. Barium Nitrate (Ba(NO₃)₂) comprises:
- 1 Barium atom
- 2 Nitrogen atoms
- 6 Oxygen atoms (since each NO₃ has 3 Oxygens and there are 2 NO₃ groups)
[tex]\[ \text{Molar mass of Ba(NO₃)₂} = 137 + 2(14) + 2(3 \times 16) = 137 + 2(14) + 2(48) = 137 + 28 + 96 = 261 \text{ g/mol} \][/tex]
### Step 2: Calculate the number of moles of barium nitrate (Ba(NO₃)₂)
Use the formula:
[tex]\[ \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} \][/tex]
Given:
- Mass of barium nitrate = 65.25 g
- Molar mass of Ba(NO₃)₂ = 261 g/mol
[tex]\[ \text{Moles of Ba(NO₃)₂} = \frac{65.25 \text{ g}}{261 \text{ g/mol}} = 0.25 \text{ moles} \][/tex]
### Step 3: Determine the number of moles of ions formed
When barium nitrate dissolves in water, it dissociates into ions. The dissociation reaction is:
[tex]\[ \text{Ba(NO₃)₂} \rightarrow \text{Ba}^{2+} + 2\text{NO}_3^- \][/tex]
From this reaction, we see:
- 1 mole of Ba(NO₃)₂ produces 1 mole of Ba²⁺ ions and 2 moles of NO₃⁻ ions.
- Therefore, for each mole of Ba(NO₃)₂, a total of 1 + 2 = 3 moles of ions are produced.
For 0.25 moles of Ba(NO₃)₂:
[tex]\[ \text{Total moles of ions} = 0.25 \text{ moles of Ba(NO₃)₂} \times 3 = 0.75 \text{ moles of ions} \][/tex]
### Conclusion:
When 65.25 g of barium nitrate dissolves in water, it forms 0.75 moles of ions.
### Step 1: Calculate the molar mass of barium nitrate (Ba(NO₃)₂)
To find the molar mass, sum up the atomic masses of all the atoms in the formula.
1. Atomic mass of Barium (Ba): 137 g/mol
2. Atomic mass of Nitrogen (N): 14 g/mol
3. Atomic mass of Oxygen (O): 16 g/mol
4. Barium Nitrate (Ba(NO₃)₂) comprises:
- 1 Barium atom
- 2 Nitrogen atoms
- 6 Oxygen atoms (since each NO₃ has 3 Oxygens and there are 2 NO₃ groups)
[tex]\[ \text{Molar mass of Ba(NO₃)₂} = 137 + 2(14) + 2(3 \times 16) = 137 + 2(14) + 2(48) = 137 + 28 + 96 = 261 \text{ g/mol} \][/tex]
### Step 2: Calculate the number of moles of barium nitrate (Ba(NO₃)₂)
Use the formula:
[tex]\[ \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} \][/tex]
Given:
- Mass of barium nitrate = 65.25 g
- Molar mass of Ba(NO₃)₂ = 261 g/mol
[tex]\[ \text{Moles of Ba(NO₃)₂} = \frac{65.25 \text{ g}}{261 \text{ g/mol}} = 0.25 \text{ moles} \][/tex]
### Step 3: Determine the number of moles of ions formed
When barium nitrate dissolves in water, it dissociates into ions. The dissociation reaction is:
[tex]\[ \text{Ba(NO₃)₂} \rightarrow \text{Ba}^{2+} + 2\text{NO}_3^- \][/tex]
From this reaction, we see:
- 1 mole of Ba(NO₃)₂ produces 1 mole of Ba²⁺ ions and 2 moles of NO₃⁻ ions.
- Therefore, for each mole of Ba(NO₃)₂, a total of 1 + 2 = 3 moles of ions are produced.
For 0.25 moles of Ba(NO₃)₂:
[tex]\[ \text{Total moles of ions} = 0.25 \text{ moles of Ba(NO₃)₂} \times 3 = 0.75 \text{ moles of ions} \][/tex]
### Conclusion:
When 65.25 g of barium nitrate dissolves in water, it forms 0.75 moles of ions.
We hope our answers were useful. Return anytime for more information and answers to any other questions you have. We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Get the answers you need at Westonci.ca. Stay informed with our latest expert advice.