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Anyway you asked the mass of sodium reacted. This is simply
Can you tell me (i) the volume of dihydrogen gas released given
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A solution of iron(III)chloride is mixed with a solution of sodium hydroxide and reacts to yield solid iron (III) hydroxide and aqueous sodium chloride. What is the balanced chemical equation for this reaction?
Start by writing the unbalanced chemical equation that describes this double displacement reaction $"FeCl"_ (3(aq)) + "NaOH"_ ((aq)) -> "Fe"("OH")_ (3(s)) darr + "NaCl"$ In order to balance...
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If 120 moles of sodium carbonate are mixed with calcium hydroxide, how many moles of sodium hydroxide are formed?
You have not told us the quantity of $"Ca(OH)"_2(aq)$ you have. $"Saturated Ca(OH)"_2(aq)$, aka $"lime water"$, does not contain a lot of . Anyway, the given equation is stoichiometrically balanced....
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A chemist performs the synthesis of sodium chloride from its elements. The chemist begins with 46 grams of sodium. How many moles of chlorine are needed?
2 Na + Cl2 → 2 NaCl
$"Moles of sodium "=(46.0*g)/(22.9*g*mol^-1)=2*mol$. Given your equation, clearly we need the ONE mole of $Cl_2$ gas. What is the mass of this quantity of chlorine? It is fact that all...
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A chemist reacted 0.05 moles of solid sodium with water to form sodium hydroxide solution. The chemical reaction for this is: Na+H2O = NaOH +H2
What mass of sodium was reacted?
Sodium has an of $22.99*g*mol^-1$. How do I know this? Well, for a start it is printed on , a copy of which will be made available in every examination...
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In the reaction $"FeC"l_2 + 2"NaOH" -> "Fe(OH)"_2"(s)" + 2"NaC"l$, if 6 moles of $"FeC"l_2$ are added to 6 moles of $"NaOH"$, how many moles of $"FeC"l_2$ would be used up in the reaction?
For any chemical reaction, the balanced chemical equation tells you the ratio that must always exist between the reactants. In your case, you have $"FeCl"_ (2(aq)) + color(blue)(2)"NaOH"_...
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What mass of sodium hydroxide ($NaOH$) is contained in 250$cm^3$ of 0.02M sodium hydroxide solution?
$"Concentration"$ $=$ $"Moles of solute"/"Volume of solution"$. And thus $"Moles of solute"="Volume of solution"xx"concentration"$. And thus $"Moles of NaOH"=250*cancel(cm^3)xx10^-3cancelL*cancel(cm^-3)xx0.02*mol*cancel(L^-1)=5.0xx10^-3*mol.$ $"Mass"="moles"xx"molar mass"=5.0xx10^-3*cancel(mol)xx40.0*g*cancel(mol^-1)=??g$
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Given a $1*L$ volume of solution that is $1.25*mol*L^-1$ with respect to $MgCl_2$, there are...?
$"a. 2 moles of ions in solution."$
$"b. 1.25 moles of ions in solution."$
$"c. 2.5 moles of ions in solution."$
$"d. 2 moles of ions in solution."$
The $"mole"$, $N_A$, is simply a number. Admittedly, it is a very large number, $N_A=6.022xx10^23*mol^-1$. And if you have a mole of stuff, you have $6.022xx10^23$ INDIVIDUAL ITEMS of that...
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How many mmols in NaOH are used? In an experiment, 5mL of 6 M NaOH is used along with 300 ml distilled water. The solution of the NaOH was titrated into a vinegar solution and it was found that 7.92 mL of NaOH was used.
The idea here is that you're diluting the stock solution to a total volume of $overbrace("5 mL")^(color(blue)("the volume of the stock solution")) + overbrace("300 mL")^(color(blue)("the volume of water"))...
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To determine the solubility of calcium hydroxide, a chemist took 25mL of a saturated calcium hydroxide solution and found that it reacted completely with 8.13mL of $0.102mol L^-1$ hydrochloric acid?
$Ca(OH)_2(aq) +2HCl(aq) rarr CaCl_2(aq) + 2H_2O(l)$ Now the calcium hydroxide present in solution derived from a saturated solution; and by saturation we specify an equilibrium quantity. That is the concentration...
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Which for the following is considered a weak base?
A. Lithium hydroxide
B. Sodium hydroxide
C. Calcium hydroxide
D. Aluminum hydroxide
Thanks!
We gots $Al(OH)_3$...even tho this is still a basic species. $"Alumina"$, $Al_2O_3$, is an amphoteric oxide...that could act as an acid. The hydroxides of lithium, calcium, or sodium, all give...
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