Answer:
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Explanation:
Answer:
Ksp = 2.4 * 10^-13
Explanation:
Step 1: Data given
Molarity of NaIO3 = 0.10 M
The molar solubility of Pb(IO3)2 = 2.4 * 10^-11 mol/L
Step 2: The initial concentration
NaIO3 = 0.1M
Na+ = 0 M
2IO3- = 0 M
Step 3: The concentration at the equilibrium
All of the NaIO3 will react (0.1M)
At the equilibrium the concentration of NaIO3 = 0 M
The mol ratio is 1:1:1
The concentration of Na+ and IO3- is 0.1 M
Pb(IO3)2 → Pb^2+ + 2IO3^-
The concentration of Pb(IO3)2 can be written as X
The concentration of Pb^2+ can be written as X
The concentration of 2IO3^- can be written as 2X
Ksp = (Pb^2+)(IO3^-)²
⇒ with (Pb^2+) = 2.4*10^-11
⇒ with (IO3^-) = 2x from the Pb(IO3)2 and 0.1M from the NaIO3.
⇒The total (IO3^-) = 2x + 0.1 and we assume that x is so small that we can neglect it.
Ksp = (2.4 *10^-11)*(0.1)²
Ksp = 2.4 * 10^-13
Hey there!:
Write the molecular equation for the reaction of MgSO4 with Pb(NO3)2 :
MgSO4(aq) + Pb(NO3)2(aq) ---> Mg(NO3)2(aq) + PbSO4(s)
Write the total ionic equation for the reaction :
Mg²⁺ (aq) + SO₄⁻² (aq) + Pb²⁺ (aq) + 2 NO₃⁻¹ (aq) + PbSO₄(s)
Therefore:
Cancel the spectator ions on both sides:
Pb²⁺ (aq) + SO₄⁻² (aq) ---> PbSO4(s)
Hope that helps!
Answer:
1.009 atm is the total pressure for the mixture
Explanation:
To determine the total pressure in atm, of the three gases (N₂, O₂ and Ar) we have to sum all the values.
Sum of partial pressures in a mixture = Total pressure
First of all, we need to convert the values from mmHg to atm
604.5 mmHg . 1atm / 760 mmHg = 0.795 atm
162.8 mmHg . 1atm / 760 mmHg = 0.213 atm
0.500 mmHg . 1atm / 760 mmHg = 6.58×10⁻⁴ atm
Partial pressure N₂ + Partial pressure O₂ + Partial pressure Ar = Total P
0.795 atm + 0.213 atm + 6.58×10⁻⁴ atm = 1.009 atm
Answer:
Explanation:
Hello!
In this case, since the percent recovery for this crystallization operation is computed as shown below:
Thus, by plugging in the initial 8.95 g and the recovered 7.20 g, we obtain:
Best regards!