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Calcium bromide speciates in aqueous solution according to the following equation.........
And thus for every metal ion there are necessarily two bromide ions.
Here by specification,
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A $2.03*g$ mass of calcium salts contains $1.33*g$ calcium carbonate. What is the $%$ calcium carbonate; and what is the percentage by mass of of calcium in calcium carbonate?
So we have the $"%calcium carbonate, "m/m$. We are not finished yet, because we have to address the percentage by mass of calcium metal in calcium carbonate: $%Ca=(40.08*g*mol^-1)/(100.09*g*mol^-1)=40%$ with respect...
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A soda bottle is flexible enough that the volume of the bottle can change even without opening it. If you have an empty soda bottle that is 2 L at room temperature of 25°C, what will the new volume be if you put it in your freezer at -4°C?
Given this proportionality, $V_1/T_1=V_2/T_2$, where $T$ is in units of $"degrees Kelvin"$, and solve for $V_2$. $"Degrees Kelvin "=" Degrees Centigrade + "273.15*K$
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Suppose 1.2 grams of calcium hydroxide are dissolved in 1.75 L of an aqueous solution. How do you determine the following: hydroxide ion concentration, hydronium ion concentration, calcium ion concentration, pH and poH?
And generally, we report $"concentration"$ with units of $mol*L^-1$. And so $[Ca(OH)_2]=((1.2*g)/(74.09*g*mol^-1))/(1.75*L)=9.26xx10^-3*mol*L^-1$. Clearly, $[HO^-]=2xx9.26xx10^-3*mol*L^-1$. Agreed? Because $[Ca(OH)_2]$ speciates in solution to give $Ca^(2+)$, and 2 equiv of hydroxide ion....
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Which solution contains the biggest amount, in mol, of chloride ions?
A. 20 cm3 of 0.50 mol dm−3 NH4Cl
B. 60 cm3 of 0.20 mol dm−3 MgCl2
C. 70 cm3 of 0.30 mol dm−3 NaCl
D. 100 cm3 of 0.30 mol dm−3 ClCH2COOH
And to answer the question, we must calculate the of of each solution with respect to chloride ions. And $"number of moles"="concentration"xx"volume"$ For $(a):$ there are $0.020*dm^3xx0.50*mol*dm^-3=0.01*mol$. For $(b):$ $0.060*dm^3xx0.20*mol*dm^-3xx"2...
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Which solution will exhibit the GREATEST freezing point depression for $1*mol*L^-1$ aqueous solutions of: $"(i) propanol; (ii) potassium bromide; (iii) calcium bromide?"$
And a colligative property depends on the NUMBER of solute particles, not their identity. Solute-solvent interactions tend to (i) INCREASE the boiling point of solutions by an amount proportional to...
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What is the concentration of $"AlF"_6^"3-"$ after mixing $"25 cm"^3$ of 0.1 mol/L aluminium ion with $"25 cm"^3$ of 1 mol/L fluoride ion?
The equilibrium is $"Al"^"3+" + "6F"^"-" ⇌ "AlF"_6^(3-)$ $K_"eq" = 1.0 × 10^25$. That means that the reaction will essentially go to completion. This becomes a limiting reactant problem....
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At some temperature, a 100-L reaction vessel contains a mixture that is initially 1.0 mol Co and 2.0 mol H2. The vessel also contains a catalyst so that the following equilibrium is attained:
CO(g) + 2H2(g) <--> CH3OH(g)
At equilibrium, the mixture contains 0.100 mol CH3OH. In a later experiment in the same vessel, you start with 1.0 mol CH3OH. How much methanol is there at equilibrium?
Methanol's concentration at equilibrium is $0.001M$. Before solving for the concentration, try and intuitively imagine what will happen. Since the second experiment is done under the same conditions as the...
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When a bottle of wine is opened, its hydrogen ion concentration, $[H_3O^+]=4.1xx10^-4*mol*L^-1$; what is its $pH$? How does the $pH$ evolve after the wine is left to stand?
And thus............when freshly opened $pH=-log_10(4.1xx10^-4)=3.39$. (And in fact most wines have a $pH$ around this level.) See on the definition of $pH$. And later $[H_3O^+]=0.0023*mol*L^-1; pH=2.64$ The wine must not...
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Calcium phosphate will precipitate out of blood plasma when calcium concentration in blood is 9.2mg/dL, and Ksp for calcium diphosphate is 8.64x10^(-13), what minimum concentration of diphospate results in precipitation?
I assume that you're actually referring to calcium diphosphate, $"Ca"_2"P"_2"O"_7$, since the question aks for the concentration of the disphosphate ions, $"P"_2"O"_7^(4-)$. Moreover, calcium phosphate, $"Ca"_3("PO"_4)_2$, has a solubility...
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What are the concentrations with respect to bromide, iodide, and hydronium ion for a solution prepared by mixing $150*mL$ of $HI(aq)$ at $0.1*mol*L^-1$ concentration, and $50*mL$ of $HBr(aq)$ at $0.05*mol*L^-1$ concentration?
And thus the total volume of solution is $(50+150)*mL$, i.e. $0.200*L.$ For each species we remember that $"concentration"="moles"/"volume"$, and thus $"number of moles"="volume"xx"concentration"$ $[I^-]=(0.150*Lxx0.1*mol*L^-1)/(0.200*L)=0.075*mol*L^-1$. $[Br^-]=(0.50*Lxx0.05*mol*L^-1)/(0.200*L)=??*mol*L^-1$. $[H_3O^+]=(0.150*Lxx0.1*mol*L^-1+0.50xx0.05*mol*L^-1)/(0.200*L)=?$.
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