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posledela
3 years ago
13

How much water, in liters, must be added to 0.5 L of 6 M HCl to make it 2 M?

Chemistry
1 answer:
barxatty [35]3 years ago
4 0
How many liters of 0.2805 M C6H12O6(aq) contain 1.000 g of C6H12O6? 
<span>a) 0.001557 L b) 0.01979 L c) 0.2805 L d) 3.565 L e) 50.5 L </span>


<span>2. If 5.15 g Fe(NO3)3 is dissolved in enough water to make exactly 150.0 mL of solution, what is the molar concentration of nitrate ion? </span>
<span>a) 0.00319 M b) 0.0343 M c) 0.142 M d) 0.313 M e) 0.426 M </span>

<span>3. What is the mass of sodium iodide in 50.0 mL of 2.63  10-2 M NaI(aq)? </span>
<span>a) 0.00132 g b) 0.00877 g c) 0.0788 g d) 0.197 g e) 78.8 g </span>

<span>4. If 25.00 mL of 4.50 M NaOH(aq) is diluted with water to a volume of 750.0 mL, what is the molarity of the diluted NaOH(aq)? </span>
<span>a) 0.0333 M b) 0.150 M c) 0.155 M d) 6.67 M e) 1.35 × 103 M </span>


<span>5. What volume of 0.15 M HCl(aq) must be diluted to make 2.0 L of 0.050 M HCl(aq)? </span>
<span>a) 0.015 L b) 0.10 L c) 0.30 L d) 0.67 L e) 6.0 L </span>

<span>6. What is the pH of 0.51 M HCl(aq)? </span>
<span>a) -0.29 b) 0.29 c) 0.31 d) 0.51 e) 0.67 </span>

<span>7. The pH of an aqueous NaOH solution is 13.17. What is the hydrogen ion concentration of this solution? </span>
a) 6.8 × 10-14 M b) 1.9 × 10-6 M c) 0.89 M d) 1.1 M e) 1. 5 × 1013 M

<span>8. The pH of a vinegar solution is 4.15. What is the H3O+ concentration of the solution? </span>
<span>a) 7.1 × 10-5 M b) 1.6 × 10-2 M c) 0.62 M d) 1.4 M e) 1.4 × 104 M </span>

<span>9. An aqueous nitric acid solution has a pH of 1.15. What mass of HNO3 is present in 2.0 L of this solution? </span>
<span>a) 0.071 g b) 0.14 g c) 2.2 g d) 4.5 g e) 8.9 g </span>

<span>10. Iron reacts with hydrochloric acid. </span>
<span>Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g) </span>
<span>What volume of 2.55 M HCl(aq) will react with 35.0 g Fe(s)? </span>
<span>a) 0.246 L b) 0.492 L c) 1.60 L d) 3.20 L e) 27.5 L </span>


<span>11. What volume of 0.200 M Na2SO4(aq) will completely react with 50.0 mL of 0.135 M Ba(NO3)2(aq)? </span>
<span>Na2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2 NaNO3(aq) </span>
<span>a) 33.8 mL b) 67.5 mL c) 74.1 mL d) 148 mL e) 540. mL </span>

<span>12. A mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq), what is the molar mass of the acid? </span>
<span>a) 2.965 × 10-3 g/mol </span>
<span>b) 9.128 g/mol </span>
<span>c) 138.7 g/mol </span>
<span>d) 337.3 g/mol </span>
<span>e) 820.7 g/mol </span>

<span>13. A 25.00 mL sample of KOH is titrated with 21.83 mL of 0.2120 M HCl(aq). What is the concentration of the KOH solution? </span>
<span>a) 0.0006720 M b) 0.002574 M c) 0.1851 M d) 0.2428 M e) 4.119 M</span>
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As the number of carbons increases in an homologous series the melting and boiling point generally_________ *
Oliga [24]
ANSWER: Increase


why? Because the number of C atoms in homologous series increases gradually.
5 0
3 years ago
Read 2 more answers
A 250.0-ml sample of ammonia, nh3 (g), exerts a pressure of 833 torr at 42.4 °c. what mass of ammonia is in the container
Lelu [443]
To solve this, let's assume ideal gas behavior.

PV=nRT
Let's solve for n. Convert units to SI units first.

Pressure = 833 torr(101325 Pa/760 torr) = 111,057.53 Pa
Volume = 250 mL(1 L/1000 mL)(1 m³/1000 L) = 2.5×10⁻⁴ m³
Temperature = 42.4 + 273 = 315.4 K

n = (8,314 J/mol·K)(315.4 K)/(111057.53 Pa)(2.5×10⁻⁴ m³)
n = 94.45 mol

The molar mass of ammonia is 17.031 g/mol.
Mass = 94.45*17.031 = <em>1,608.51 g ammonia</em>


6 0
4 years ago
What is the mass of carbon in 500. g of octane?
denis23 [38]

The answer is: the mass of carbon is 420.6 grams.

m(C₈H₁₈) = 500 g; mass of octane.

M(C₈H₁₈) = 114.22 g/mol; molar mass of octane.

n(C₈H₁₈) = m(C₈H₁₈) ÷ M(C₈H₁₈).

n(C₈H₁₈) = 500 g ÷ 114.22 g/mol.

n(C₈H₁₈) = 4.38 mol; amount of octane.

In one molecule of octane, there are eight carbon atoms:

n(C) = 8 · n(C₈H₁₈).

n(C) = 8 · 4.38 mol.

n(C) = 35.02 mol; amount of carbon.

m(C) = 35.02 mol · 12.01 g/mol.

m(C) = 420.6 g; mass of carbone.

5 0
4 years ago
CdF2(s)⇄Cd2+(aq)+2F−(aq)A saturated aqueous solution of CdF2 is prepared. The equilibrium in the solution is represented above.
kupik [55]

Answer:

The correct answer is option a.

Explanation:

CdF_2(s)\rightleftharpoons Cd^{2+}(aq)+2F^-(aq)

Equilibrium concentration cadmium ions = [Cd^{2+}]=0.0585 M

Equilibrium concentration fluoride ions = [F^{-}]=0.117 M

Molar solubility is the maximum concentration of salt present in water in ionic form beyond that no more salt will exist in its ionic form and will settle down in bottom of the solution.

The molar solubility of the solid cadmium fluoride = 0.0585 M

CdF_2(s)\rightleftharpoons Cd^{2+}(aq)+2F^-(aq)..[1]

NaF(s)\rightleftharpoons Na^{+}(aq)+F^-(aq)

Due to addition of sodium fluoride will increase concentration of fluoride in the solution.And due to common ion effect the equilibrium will shift in backward direction in [1], that is precipitation of more cadmium fluoride.

Hence, decrease in solubility will be observed.

8 0
3 years ago
How do you tell if elements have similar chemical properties periodic table?
Oksi-84 [34.3K]
Whether or not they are within the same group (vertical columns) within the periodic table, determines similarity of chemical properties.
5 0
3 years ago
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