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Alexxandr [17]
3 years ago
5

What is the possible results of the test of a few drops of a mixture of sodium hydroxide and copper(ii) tetraoxosulphate (vi) so

lution added to a sample of urine test in a test tube
Chemistry
1 answer:
8090 [49]3 years ago
4 0

Answer:

The urine may turn purple or remain colourless

Explanation:

Adding sodium hydroxide (NaOH) and hydrated copper(II) sulfate to urine in a test tube is a test for proteins in urine.

This test depends on the ability of sodium hydroxide (NaOH) and hydrated copper(II) sulfate to form purple-coloured cordination complexes with peptides. The appearance of this purple colour is a positive test for protiens in urine.

Hence, when a few drops of a mixture of sodium hydroxide and copper(ii) tetraoxosulphate (vi) solution added to a sample of urine test in a test tube, the solution may turn purple indicating the presence of proteins in urine or remain colourless indicating the absence of proteins in urine.

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It's probably animal if that's what's you're asking.
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How many moles can be found in 1.5 x 10^24 atoms of Calcium?
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2.49 x 10^46 is the answer
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Still using the reaction from the video, what is the limiting reagent when 2 moles of Al are reacted
kondaur [170]

The limiting reagent will be Al

<h3>What are limiting reagents?</h3>

They are reagents that limit the quantity of products that are formed in reactions.

From the equation of the reaction:

4Al + 3O_2 --- > 2Al_2O_3

The mole ratio of Al to O2 is 4:3.

With 2 moles of Al and 2 moles of O2, Al becomes limiting while O2 is in excess.

With 2 moles of O2, the amount of Al required should be:

                          2 x 4/3 = 2.67 moles.

With 2 moles of Al, the amount of O2 required should be:

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Thus, O2 is in excess by 0.5 moles.

More on limiting reagents can be found here: brainly.com/question/11848702

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8 0
2 years ago
An aqueous solution is listed as being 33.8% solute by mass with a density of 1.15 g/mL, the molar mass of the solute is 145.6 g
vodomira [7]

Answer:

A) 2.69 M

B) 0.059

Explanation:

A) We have:

33.8% solute by mass= 33.8 g solute/100 g solution

molarity = mol solute/ 1 L solution

molarity= \frac{33.8 g solute}{100 g solution} x \frac{1.15 g solution}{1 ml} x \frac{1 mol solute}{145.6 g solute} x \frac{1000 ml}{1 L}

molarity= 2.69 mol solute/L solution = 2.69 M

B) We know that there are 33.8 g of solute in 100 g of solution.

As the total solution is compounded by solute+solvent (in this case, solvent is water), the mass of water is the difference between the mass of the total solution and the mass of solute:

mass of water= 100 g - 33.8 g = 66.2 g

Now, we calculate the number of mol of both solute and water:

mol solute= 33.8 g solute x \frac{1 mol solute}{145.6 g} = 0.232 mol

mol H20= 66.2 g H₂O x \frac{1 mol H2O}{18 g}

Finally, the mol fraction of solute (Xsolute) is calculated as follows:

Xsolute=\frac{mol solute}{total mol}= \frac{mol solute}{mol solute + mol H2O}=\frac{0.232 mol}{0.232 mol + 3.677 mol}

Xsolute= 0.059

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