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an excess of copper(II) oxide is reacted with 1.0 mol dm3 sulphuric acid. Calculate the volume of sulphuric acid needed to prepare 20.0 g of copper(II) sulphate.
For the reaction of cupric oxide with sulfuric acid, the balanced chemical equation is CuO plus H₂SO₄ react to form CuSO₄ plus H₂O.
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What volume of a 0.126 M potassium hydroxide solution is required to neutralize 22.0 mL of a 0.139 M nitric acid solution? ___________mL potassium hydroxide
v=0.139/22=0.006molV=0.126/0.006=21ml
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The commercial sulphuric acid solution includes 96.4 % H2SO4 by mass. The density of the solution is 1.84 g/mL. Calculate the molarity of the sulphuric acid solution?
Molecular weight of H2SO4 is 98.079 g-mol.1 ml equals 1.84 g. Hence, 96.4ml equals 96 x 1.84 = 177.376g.Therefore, 100 ml volume contains 177.376 g H2SO4. So 1 liter contains...
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Sulphuric acid reacts with potassium to form potassium sulphate and hydrogen. Determine the mass of potassium sulphate produced if 6.0g of hydrogen wa also formed
2K + H2SO4 = K2SO4 + H2 if m(H2) = 6 g, so n(H2) = 6 g / 2 g/mol = 3 moles; n(H2) : n(K2SO4) = 1 : 1;...
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Find the molarity and molality of a 15% solution of sulphuric acid whose density is 110g/cc and the molar mass of the sulphuric acid is 98g/mol
110 g/cc is larger than the density of iridium. Certainly you meant 1.10 g/cc. To ease the calculations, take 1 liter of the solution. Its mass is m = V*D...
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What mass of ethanol is needed to create 2.5 gram of ethanoic acid (CH3COOH)? assume the ratio of ethanol to ethanoic acid needed is 1:1
m(CH3CH2OH) = 2,5g n(CH3CH2OH) : n(CH3COOH) = 1: 1 m(CH3COOH) = ? X g 2.5g CH3CH2OH → CH3COOH 46 g/moll 60 g/moll 46g (CH3CH2OH) ─ 60g (CH3COOH) X g (CH3CH2OH)...
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63.9 ml of 0.560 M sulfuric acid solution was completely neutralized by 28.3 ml of potassium hydroxide solution. What was the concentration of the potassium hydroxide?
Reaction of neutralization of sulfuric acid by potassium hydroxide: H_2 SO_4+2KOH=K_2 SO_4+H_2 O Using the Law of equivalence: n(H_2 SO_4 )=n(KOH) c(H_2 SO_4 )∙V(H_2 SO_4 )=c(KOH)∙V(KOH) c(KOH)=(c(H_2 SO_4 )∙V(H_2 SO_4...
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Sulphuric acid has a molecular mass of 98 and a density of 1.94 g/mL. You are given a 10% v/v solution of sulphuric acid. What is its molar concentration? Give your answer to 2 decimal places.
If we have 1L of solution, then we have 100 ml (0.1L = 10% from 1L) of sulphuric acid in it. Find the mass of 100 ml of sulphuric acid:...
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What volume of a 0.171 M barium hydroxide solution is required to neutralize 24.0 mL of a 0.225 M hydrobromic acid solution?
_________ mL barium hydroxide
xmol 0.0054molBa(OH)2 + 2HBr = BaBr2 +2H2O 1mol 2mol n(HBr) = C(HBr) × V(HBr) = 0.225M × 0.024L = 0.0054mol.n(Ba(OH)2) = x = 0.0054 × 1 / 2 mol = 0.0027mol.V(Ba(OH)2) = n(Ba(OH)2) /...
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How much potassium hydroxide is needed to make 1.00 liter of a 0.5 Molar solution of potassium hydroxide ?
Solution: C(KOH) = n(KOH)/V(solution)n(KOH) = C(KOH)*V(KOH) = 0.5 M* 1L = = 0.5 molm(KOH)= n(KOH)*M(KOH) = 0.5 mol*56 g/mol = 28 g
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