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3 years ago

Which compound is an electrolyte? (1) C6H12O6 (3) CaCl2 (2) CH3OH (4) CCl4

1 answer:

4 0

I think the correct answer is option 3. CaCl2 is the compound that is an electrolyte when dissolved in water. An electrolyte is a substance that conducts electricity in solution. Calcium Chloride when in solution dissociates into ions which allows the flow of current in the solution.

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Identify the compound whose solubility decreases with increasing temperature.

Veronika [31]

Answer is: Na₂SO₄ (sodium sulfate).

The solubility of sodium sulfate increases up to 32.38°C and than decreases at higher temperatures, the solubility becomes almost independent of temperature.

At 32.38°C it releases of crystal water and melting of the hydrated salt.

Sodium sulfate is the white, inorganic compound.

Sodium sulfate is highly soluble in water.

5 0

3 years ago

Which element do all organic compounds contain?

bulgar [2K]

Answer:

hydrogen oxygen or nitrogen

6 0

3 years ago

You notice that the water in your friend's swimming pool is cloudy and that the pool walls are discolored at the water line. A q

Flauer [41]

Answer:

6,78 mL of 12,0 wt% H₂SO₄

Explanation:

The equilibrium in water is:

H₂O (l) ⇄ H⁺ (aq) + OH⁻ (aq)

The initial concentration of [H⁺] is 10⁻⁸ M and final desired concentration is [H⁺] = $10^{-7,20}$ , thus,

Thus, you need to add:

[H⁺] = $10^{-7,2} -10^{-8,0}$ = 5,31x10⁻⁸ M

The total volume of the pool is:

9,00 m × 15,0 m ×2,50 m = 337,5 m³ ≡ 337500 L

Thus, moles of H⁺ you need to add are:

5,31x10⁻⁸ M × 337500 L = 1,792x10⁻² moles of H⁺

These moles comes from

H₂SO₄ → 2H⁺ +SO₄²⁻

Thus:

1,792x10⁻² moles of H⁺ × $\frac{1H_{2}SO_4 mol}{2H^{+} mol}$ = 8,96x10⁻³ moles of H₂SO₄

These moles comes from:

8,96x10⁻³ moles of H₂SO₄ × $\frac{98,1 g}{1 mol}$ × $\frac{100 gSolution}{12 gH_{2}SO_4 }$ × $\frac{1 mL}{1,080 g}$ =

6,78 mL of 12,0wt% H₂SO₄

I hope it helps!

8 0

3 years ago

Write the formulas for the following ionic compounds: (a) copper bromide (containing the Cu+ ion), (b) manganese oxide (containi

ivann1987 [24]

Answer:The formulas of ionic compounds are:

a) $CuBr$

b) $Mn_2O_3$

c) $Hg_2I_2$

d) $Mg_3(PO_4)_2$

Explanation:

Formulas for the an ionic compounds is determine by:

Criss-cross method, the oxidation state of the ions gets exchanged and they form the subscripts of the other ions. This results in the formation of a neutral compound.

(a) Copper bromide :Given that it contains $Cu^+$ ion.

$Cu^++Br^-\rightarrow CuBr$

(b) Manganese oxide : Given that it contains $Mn^{3+}$ ion.

$Mn^{3+}+O^{2-}\rightarrow Mn_2O_3$

(c)Mercury iodide :Given that it contains $Hg_2^{2+}$

$Hg_2^{2+}+I^-\rightarrow Hg_2I_2$

(d) Magnesium phosphate :Given that it contains $PO_4^{3-}$

$Mg^{2+}+PO_4^{3-}\rightarrow Mg_3(PO_4)_2$

4 0

3 years ago

1. Calculate how many moles of glycine are in a 130.0-g sample of glycine.2. Calculate the percent nitrogen by mass in glycine.

Alexxx [7]

Answer:

$n=1.732mol$

$\% N=18.7\%$

Explanation:

Hello!

In this case, since the molecular formula of glycine is C₂H₅NO₂, we realize that the molar mass is 75.07 g/mol; thus, the moles in 130.0 g of glycine are:

$n=130.0g*\frac{1mol}{75.07 g}\\\\ n=1.732mol$

Furthermore, we can notice 75.07 grams of glycine contains 14.01 grams of nitrogen; thus, the percent nitrogen turns out:

$\% N=\frac{14.01}{75.07}*100\% \\\\\% N=18.7\%$

Best regards!

4 0

3 years ago