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I will assume you don't need this solved, but want a starting point since that is what you're asking.
To calculate the moles of propanoic acid, we do a simple stoichiometric calculation,
The same goes for the initial hydroxide added.
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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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How do I find the mass of copper(II) hydroxide which is formed when excess copper(II) sulfate is added to 100mL of a 0.450 mol $L^-1$ solution of sodium hydroxide?
An alternative approach is to simply use the that exist between the species that take part in the reaction, then use the molar mass of copper(II) hydroxide, $"Cu"("OH")_2$, to get...
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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...?
$"a. 2 moles of ions in solution."$
$"b. 1.25 moles of ions in solution."$
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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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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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How many moles of sodium hypochlorite should be added to 1L of 0.05M hypochlorous acid to form a buffer solution with pH 9.15ssume no changes of volume occurs when NaOCl salt is added?
First thing first - you need to know the acid dissociation constant for hypochlorous acid, $"HClO"$, which is listed as being equal to $K_a = 3.0 * 10^(-8)$...
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A given volume of a buffer solution contains $6.85 x 10^-3$ mol of the weak acid HY and $2.98 x 10^-3$ mol of the salt NaY. The pH of the buffer solution is 3.78. How do you calculate the value of $pKa$ for the acid HY at this temperature?
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What is the $pH$ of a buffer solution prepared from $50*mL$ of sodium hydroxide solution that is $0.220*mol*L^-1$ with respect to $NaOH$, and $100*mL$ of acetic acid solution that is $0.150*mol*L^-1$ with respect to $HOAc$?
We use the buffer such that, $pH=pK_a+log_10{[[""^(-)OAc]]/[[HOAc]]}$ But of course, we have to calculate $[""^(-)OAc]$ and $[HOAc]$. The volume of the solution is clearly $150*mL$. $"Moles of NaOH"-=(50.0xx10^-3Lxx0.220*mol*L^-1)=0.011*mol.$ $"Moles of...
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How do I calculate the $"pH"$ of the buffer solution formed when $10.0$ $"cm"^3$ of $0.80$ $"mol"$ $"dm"^-3$ sodium hydroxide is mixed with $50.0$ $"cm"^3$ of $0.50$ $"mol"$ $"dm"^-3$ ethanoic acid ($"K"_"a"=1.74xx10^-5$ $"mol"$ $"dm"^-3$)?
The first thing you must recognize is that there will be an acid-base reaction. Your first task is to calculate the concentrations of the species present at the end of...
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