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A saturated solution of lead(ll) nitrate was made at 50°C using 100 g of water, and this was then allowed to cool to 30 °C. What would happen as the solution cooled?
You have described the formation of a saturated solution of $Pb(NO_3)_2$. If the solution is saturated, then it contains the same amount of that would be in equilibrium with undissolved...
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If 55 grams of $KCl$ are dissolved in 100 grams of water at 80°C is the solution saturated unsaturated, or supersaturated?
$"Saturation"$ defines an equilibrium condition. Namely that a $"saturated solution"$ is a solution that contains an amount of equal to that amount of solute that would be in equilibrium with...
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A solution is prepared by dissolving 3.5 $g$ of $KCl$ in water & making the volume of solution to 250 $mL$. What is the millimoles of $KCl$ dissolved?
To calculate how many milimoles of potassium chloride you dissolved in solution, all you really need to do is figure out how many moles of the salt you used....
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A 5.00 mL sample of a solution of KCl (Mwt=74.6 g/mol) in water (Mwt=18.01 g/mol) weighs 5.20 g. The water is evaporated off leaving 0.26 g of residue. What is the mass of solution that would contain 1.00 g of KCl?
The first thing you need to do here is to figure out the of the solution, $rho$, by using its mass, $m$, and its volume, $V$ $color(blue)(ul(color(black)(rho =...
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A certain amount of rubidium iodide was dissolved in $"4.6 L"$. A $"1-L"$ aliquot was extracted an diluted to $"13.9 L"$ to form a $"0.65 M"$ solution in water. What mass of rubidium iodide was dissolved into the original solution?
For this kind of questions, we use the formula: $("mol")/("volume "color(blue)("L"))="concentration " color(blue)("mol"xx"L"^-1)$ To calculate the mass of rubidium iodide ($RbI$), we need to calculate back to the original solution....
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Urea, $("NH"_2)_2"CO"$, is dissolved in $"100 g"$ of water. The solution freezes at $-0.085^@"C"$. How many grams of urea were dissolved to make this solution?
Your tool of choice here will be the equation that allows you to calculate the freezing point depression of the solution $color(blue)(ul(color(black)(DeltaT_"f" = i * K_f * b)))$...
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Could you help me with this? Justify the statement with an example: "Formality does not depend on what happens to a solute after it is dissolved in water, but depends on amount of solute dissolved in water."
and formality both express a solution's concentration as the ratio between the moles of and the liters of solution. However, formality does not depend on what happens...
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What molar quantity of ions are realized in solution when a $0.50*mol$ quantity of $Cr_2(SO_4)_3$ is dissolved in water? What about when a $0.50*mol$ quantity of $Rb_3(PO_4)_3$ is dissolved?
$Cr_2(SO_4)_3(s) rarr 2Cr^(3+) + 3SO_4^(2-)$ Thus 5 moles of ions result from one mole of solute. We started with half a mole of solute, and thus 2.5 mole ions result....
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When $1.0$ $g$ of potassium chloride, $KCl$, is dissolved in $25$ $mL$ (=$25$ $g$) of water, it causes the temperature to drop from $24.33^o$ $C$ to $22.12^o$ $C$. What is the molar enthalpy of dissolution for $KCl$?
The reaction in question is: $KCl_"(s)" to K^"+"(aq) + Cl^"-" (aq)$ The reaction is endothermic, so the value of $Delta H$ we calculate at the end will be positive....
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A 29.80 g sample of liquid cadmium at 377.00°C is poured into a mold and allowed to cool to 24.00°C. How many kJ of energy are released in this process?
Since you calcium starts this process at 377 °C and is in liquid phase, the heat of vapourization does not enter into this. However, the heat of fusion does, as...
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