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Rudik [331]
3 years ago
10

En el laboratorio, un vaso precipitado vacío tiene una masa de 0,50 kg. Este vaso se llena con 300 cm3 de una solución saturada

con sacarosa, llegando a tener el vaso una nueva masa de 730 g. ¿Cuál será la densidad de la solución en el vaso?
Chemistry
1 answer:
faust18 [17]3 years ago
4 0

Answer:

Density = 0.0007667 Kg/cm³

Explanation:

Given the following data;

Mass of empty beaker = 0.50 kg

Volume of solution = 300 cm³

Mass of glass+solution = 730 g

To find the density of the solution in the glass;

First of all, we would convert the value in grams to kilograms.

Conversion:

1000 grams = 1 kg

730 = X kg

Cross-multiplying, we have;

X = 730/1000 = 0.73 kg

Next, we would determine the mass of the solution.

Mass of solution = Mass of glass+solution - Mass of empty beaker

Mass of solution = 0.73 - 0.50

Mass of solution = 0.23 kg

Lastly, we would solve for the density of the solution;

Density can be defined as mass all over the volume of an object.

Simply stated, density is mass per unit volume of an object.

Mathematically, density is given by the formula;

Density = \frac {mass}{volume}

Substituting into the formula, we have;

Density = \frac {0.23}{300}

Density = 0.0007667 Kg/cm³

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The table below shows the volume of two samples, A and B, when placed in three containers of different volumes.
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7 0
2 years ago
Read 2 more answers
Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions: Zn2+, Ni4+, F-
hram777 [196]

Ionic compounds are formed between oppositely charged ions.

A binary ionic compound is composed of ions of two different elements - one of which is a positive ion(metal), and the other is negative ion (nonmetal).

To write the empirical formula of binary ionic compound we must remember that one ion should be positive and other ion should be negative, then only the correct formula should be written. To write the empirical formula the charges of opposite ions should be criss-crossed.

First empirical formula of binary ionic compound is written betweenZn^{2+} (Positive ion)and F^{-} (Negative ion)

First Formula would be ZnF_{2}

Second empirical formula is between Zn^{2+}(Positive ion) and O^{2-}(Negative ion)

Second Formula would be Zn_{2}O_{2}

Note : When the subscript are same they get cancel out, so Zn_{2}O_{2} would be written as ZnO

Third empirical formula is between Ni^{4+}(Positive ion) and F^{-}(Negative ion)

Third Formula would be :NiF_{4}

Forth empirical formula is between Ni^{4+}(Positive ion)and O^{2-}(negative ion)

Forth Formula would be : Ni_{2}O_{4} or NiO_{2}

Note- The subscript will be simplified and the formula will be written as NiO_{2}.

The empirical formula of four binary ionic compounds are : ZnF_{2}, ZnO, NiF_{4},NiO_{2}


8 0
2 years ago
Read 2 more answers
What is the oxidation number of cl− in the hypochlorite ion clo−?
mariarad [96]

Answer : The oxidation number of chlorine (Cl) is, (+1)

Explanation :

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Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

When the atoms are present in their elemental state then the oxidation number will be zero.

Rules for Oxidation Numbers :

The oxidation number of a free element is always zero.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of  Hydrogen (H)  is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of  oxygen (O)  in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

The given compound is, ClO^-

Let the oxidation state of 'Cl' be, 'x'

x+(-2)=-1\\\\x-2=-1\\\\x=+1

Therefore, the oxidation number of chlorine (Cl) is, (+1)

5 0
3 years ago
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