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2 years ago

A solution is made by mixing 15.0 g of sr(oh)2 and 55.0 ml of 0.200 m hno3.

Chemistry

1 answer:

noname [10]2 years ago

4 0

Letter A: The balanced equation is:

Sr(OH)2 (s) + 2 HNO3 (aq) → Sr(NO3)2 (aq) + 2 H2O

Letter B: The solution is:

(15.0 g Sr(OH)2) / (121.6358 g Sr(OH)2/mol) = 0.12332 mol Sr(OH)2
(0.0550 L) x (0.200 mol/L HNO3) = 0.011 mol HNO3

0.011 mole of HNO3 would respond entirely with 0.011 x (1/2) = 0.0055 mole of Sr(OH)2 but there is more Sr(OH)2 existing than that, so Sr(OH)2 is in excess and HNO3 is the limiting reactant.

( 0.011 mol HNO3) x (1/2) = 0.0055 mol Sr(NO3)2

Since the NO3{-} ions continued in solution during, the concentration of the NO3{-} ions didn't change during the reaction, so they are still 0.200 M.
The concentration of Sr{+2} ions is (0.0055 mol Sr(NO3)2) / (55.0 mL) = 0.100 M
Since HNO3 is the limiting reactant, no H{+} ions continue at the end of the reaction.

Letter C: Since all of the acid reacted and there was still Sr(OH)2 left over, the resulting solution would be basic.

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Natali5045456 [20]

Answer:

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Explanation:

Given data:

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Final temperature = 35°C (35+273 = 308 k)

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Mathematical expression:

V₁/T₁ = V₂/T₂

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T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

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2 years ago

820 g Li2SO4 is dissolved into 2500 mL of solution. What is the molar concentration?

Andreas93 [3]

Molarity is defined as the moles of solute per liter of solution. $M=\frac{n}{V}$ . Where M is molarity, n is the number of moles and V is the volume. First we must find the molar mass of $Li_2SO_4$ which is 109.98 g/mol

$Li_2SO_4= 2 \times Li_{Ar} + S_{Ar} + 4 \times O_{Ar}\\= (2 \times 6.941 + 32.1 + 4 \times 16.0) = 109.98 g/mol$

$820\ g\ Li_2SO_4 \times \frac{mol}{109.98\ g}= 7.46\ mol\ Li_2SO4$

Then we find the molarity using above equation

$M= \frac{n}{V} = \frac{7.46 mol}{2500ml} \times\frac{1000ml}{L} = 2.98\ M$

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3 years ago

What is the volume of 1.50 lb (pounds) of mercury? The density of mercury is 13.546 g/mL. Use the conversion that 1 kg = 2.20 lb

Arada [10]

Answer:

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Explanation:

Punds are an unit of mass. To convert mass to volume we must use density (13.546g/mL). Now, As you can see, density is in grams but the mass of mercury is in pounds. That means we need first, to convert pounds to grams to use density and obtain volume of mercury.

Mass mercury in grams:

1.50lb * (1kg / 2.20lb) = 0.682kg = 682g of mercury.

Volume of mercury:

682g Mercury * (1mL / 13.546g) =

<h3>50.3mL of mercury are in 1.50lb</h3>

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2 years ago

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PilotLPTM [1.2K]

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2 years ago

Read 2 more answers

When 4.5 mol al react with 11.5 mol hcl, what is the limiting reactant, and how many moles of h2 can be formed?

ahrayia [7]

1°/ . 2 Al + 6 HCl → 2 AlCl3 + 3 H2

k1 = n(Al) / 2 = 4,5 / 2 = 2,25 
k2 = n(HCl) / 6 = 11,5 / 6= 1,92 

k2 < k1 ==> HCl is the limiting reactant 

6 mol of HCl ---> 2 mol of H2 
11,5 mol of HCl ---> 3,83 mol of H2

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2 years ago