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MrRissso [65]
3 years ago
9

How many grams of solid barium sulfate form when 25.0 ml of 0.160 m barium chloride reacts with 68.0 ml of 0.055 m sodium sulfat

e? bacl2(aq) + na2so4(aq) --> baso4(s) + 2nacl(aq)?

Chemistry
1 answer:
GalinKa [24]3 years ago
8 0
Hope this will help you.

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What is number 2? the brain stem......
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3 years ago
A hydrated blue copper(II) sulfate salt with a formula YCuSO4•XH2O is heated until it is completely white in color. The student
Mariulka [41]

Answer:

X = 5

Explanation:

The molar ratio of water to copper(II) sulfate must be found.

The mass of water that must have been eliminated from the salt is found by the difference in weight before and after:

(500 g) - (320 g) = 180 g water eliminated

The moles of water (MW 18.02 g/mol) is then found:

(180 g) / (18.02g/mol) = 9.9889...mol

The mass of the dehydrated copper(II) sulfate (MW 159.609 g/mol) is converted to moles:

(320 g) / (159.609 g/mol) = 2.004899...mol

The molar proportion of water to the copper(II) sulfate is then calculated:

(9.9889...mol H₂O) / (2.0034899...mol CuSO₄) ≅ 5

3 0
3 years ago
Please help me out...
liq [111]

Answer:

Explanation:

To convert from grams to atoms, first divide by the molar mass, the multiply by 6.022*10^23.

To convert from moles to mass, multiply by the molar mass of the element.

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2 years ago
Sometimes, during the DNA replication process, mistakes are made. These are called
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3 years ago
Read 2 more answers
How many grams are in 5.2 moles of Li2SO4
skelet666 [1.2K]

Answer:

572 g

Explanation:

Molar mass is the mass of 1 mol of an element or compound

molar mass of Li₂SO₄ is the sum of the products of the molar masses of the elements by the number of atoms in the compound

molar masses of each element making up lithium sulphate

Li - 7 g/mol

S - 32 g/mol

O - 16 g/mol

molar mass of Li₂SO₄ - (7 g/mol x 2) + ( 32 g/mol x 1) + ( 16 g/mol x 4 )

molar mass = 110 g/mol

mass of 1 mol of Li₂SO₄ is 110 g

therefore mass of 5.2 mol of Li₂SO₄ is - 110 g/mol x 5.2 mol = 572 g

mass is 572 g

7 0
3 years ago
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