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MrRa [10]
2 years ago
12

Write ionic equations for the following: HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)

Chemistry
1 answer:
vodomira [7]2 years ago
4 0

Answer:

HCl(aq) + KOH(aq) ===> H2O(l) + KCl(aq)

Note the stoichiometry of the balanced equations shows us that HCl and KOH react in a 1:1 mole ratio. So, let us find moles of HCl and moles of KOH that are present:

moles HCl = 250.0 ml x 1 L/1000 ml x 0.25 mol/L = 0.06250 moles HCl

moles KOH = 200.0 ml x 1 L/1000 ml x 0.40 mol/L = 0.0800 moles KOH

You can see that there are more moles of KOH than there are of HCl, meaning that KOH is in excess and after neutralizing all of the HCl, the solution will be left with excess KOH making the pH > 7 = BASIC

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What is the ∆G for the following reaction between O3 and O2? 3O2(g) 2O3(g) Given: O3: ∆H = 285.4 kJ ∆S = -137.14 J/K)
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We’ll be using the equation:
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What mass of Calcium Bromide (below) is needed to make 0.500 L of
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55.36 is the mass of Calcium Bromide is needed to make 0.500 L of  0.554 M solution.

Explanation:

Data given:

mass of CaBr_{2} = ?

molarity of the calcium bromide solution = 0.554 M

Volume of the calcium bromide solution= 0.5 L

First the moles of calcium bromide is calculated as:

molarity = \frac{number of moles}{volume in litres}

number of moles = 0.554 x 0.5

number of moles = 0.277 moles of calcium bromide

atomic mass of calcium bromide = 199.89 grams/mole

mass = atomic mass x number of moles

mass of calcium bromide = 199.89 x 0.277

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mass of calcium bromide required is 55.36 grams to make solution of 0.554 M in a solution of 0.5 litres.

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