For parts a and b, explain why the substances follow (or do not follow) the law of multiple proportions. take m(o) = 16 g/mol, m(mn) = 55 g/mol, and m(i) = 127 g/mol and derive the empirical formulae of all mentioned compounds. part a. sample a of manganese (mn) oxide contains 330 mg of mn and 144 mg of o, sample b — 330 mg of mn and 336 mg of o. part b. sample a of iodine (i) oxide contains 508 mg of i and 128 mg of o, sample b — 508 mg of i and 144 mg of o.

2. part a. calculate the mass of barium chloride dihydrate required to prepare a 1.500 l solution of 0.1500 mol/l ba2+. m(bacl2·2h2o) = 244.26 g/mol. part b. calculate the mass of copper(ii) sulfate pentahydrate required to prepare a 2.500 l solution of 0.2500 mol/l cu2+. m(cuso4·5h2o) = 249.69 g/mol.

Answers are in the explanation.

Explanation:

The law of multiple propotions says that "when two elements combine with each other to form more than one compound, the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers". Using this law it is possible to obtain empirical formula of the compounds, thus:

1. A, sample A.

0,330g Mn× = 6x10⁻³ moles

0,144g O× = 9x10⁻³ moles

Ratio O:Mn = 9x10⁻³ / 6x10⁻³ = 1,5

To explain this ratio, empirical formula must be:

Mn₂O₃

1. A, sample B.

0,330g Mn× = 6x10⁻³ moles

0,336g O× = 2,1x10⁻² moles

Ratio O:Mn = 2,1x10⁻² / 6x10⁻³ = 3,5

To explain this ratio, empirical formula must be:

Mn₂O₇

1. B, sample A.

0,508g I× = 4x10⁻³ moles

0,128g O× = 8x10⁻³ moles

Ratio O:Mn = 8x10⁻³ / 4x10⁻³ = 2

To explain this ratio, empirical formula must be:

I₂O

1. B, sample B.

0,508g I× = 4x10⁻³ moles

0,144g O× = 9x10⁻³ moles

Ratio O:Mn = 9x10⁻³ / 4x10⁻³ = 2,25

To explain this ratio, empirical formula must be:

I₉O₄

2. Part A.

1,5L solution×× = 54,96g of BaCl₂.2H₂O

2. Part B.

2,5L solution×× = 156,1g of CuSO₄.5H₂O

I hope it helps!

i think it is true since you can test the answer and can use observations to complete it.

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.