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yuradex [85]
3 years ago
11

.22

Chemistry
2 answers:
Alja [10]3 years ago
7 0

Answer:its b

Explanation:

andriy [413]3 years ago
5 0

Answer:

(a)  

First, write the balanced equation as follows:

Na2S(aq) + ZnCl2(aq) -> 2 NaCl(aq) + ZnS  (s)

Then, rewrite the equation so that all dissolved compounds are separated into their constituted ions. This is called, total ionic equation:

2 Na^+(aq) + S^{2-}(aq) + Zn^{2+}(aq) + 2 Cl^-(aq) -> ZnS (s) + 2 Na^+(aq) + 2 Cl^-(aq)

Finally, cancel the ions that appear both in reactants and products. This is called, net ionic equation:

S^{2-}(aq) + Zn^{2+}(aq) -> ZnS (s)

(b)

Balanced equation:

2 K3PO4(aq) + 3Sr(NO3)2(aq) -> Sr3(PO4)2 (s) + 6 KNO3 (aq)

Total ionic equation:

6 K^+(aq) + 2 PO_4^{3-} (aq) + 3 Sr^{2-} (aq) + 6 NO_3^- (aq) -> Sr3(PO4)2 (s) + 6 K^+(aq) + 6 NO_3^- (aq)

Net ionic equation:

2 PO_4^{3-} (aq) + 3 Sr^{2-} (aq) -> Sr3(PO4)2 (s)

(c)

Balanced equation:

Mg(NO3)2(aq) + 2NaOH(aq) -> Mg(OH)2 (s) + 2 NaNO3 (aq)

Total ionic equation:

Mg^{2+} (aq) + 2 NO_3^- (aq) + 2 Na^+ (aq) + 2 OH^- (aq) -> Mg(OH)_2 (s) + 2 NO_3^- (aq) + 2 Na^+ (aq)

Net ionic equation:

Mg^{2+} (aq) + 2 OH^- (aq) -> Mg(OH)_2 (s)

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What is the empirical formula of a compound that is 24.42 % calcium, 17.07 % nitrogen, and 58.5% oxygen?
REY [17]

Answer:

CaN_{2} O_{6}

Explanation:

When calculating an empirical formula from percentages, assume you have a 100g sample. This allows you to convert the percentages directly to grams, because X % of 100g is X grams.

So:

24.42 % = 24.42 g Ca, 17.07% = 17.07g N, 58.5% = 58.5g O

The next step is to divide each mass by their molar mass to convert your grams to moles.

24.42/40.08 = 0.6092 mol

17.07/14.01 = 1.218 mol

58.85/15.99 = 3.680 mol

Then you will divide all of your mol values by the SMALLEST number of moles. This gives you whole numbers that are the mole ratio (subcripts) of the empircal formula.

0.6092 mol/0.6092 mol = 1

1.218 mol/0.6092 mol = 2

3.680 mol/0.6092 mol = 6

So the empirical formula is CaN_{2} O_{6}

5 0
3 years ago
What is the pH of a solution that has a pOH of 5.9
Stella [2.4K]

Answer:

pH = 8.1

Explanation:

Assuming that we are at 25 degrees Celsius, pH + pOH = 14.

We can then plug in the given pOH and solve for pH:

pH + pOH = 14

pH + 5.9 = 14

pH = 14 - 5.9 = 8.1

7 0
3 years ago
Which is stronger - the attractive forces between water molecules and chromium and chloride ions, or the combined ionic bond str
Tju [1.3M]

Answer is: the combined ionic bond strength of CrCl₂ and intermolecular forces between water molecules.

When chromium chloride (CrCl₂) is dissolved in water, the temperature of the water increases, heat of the solution is endothermic.

Dissociation of chromium chloride in water: CrCl₂(aq) → Cr²⁺(aq) + 2Cl⁻(aq).

Energy (the lattice energy) is required to pull apart the oppositely charged ions in chromium chloride.

The heat of hydration is liberated energy when the separated ions (in this example chromium cations and chlorine anions) attract polar water molecules.

Because the lattice energy is higher than the heat of the hydration (endothermic reaction), we can conclude that bonds between ions are strong (the electrostatic attraction between oppositely charged ions).

3 0
3 years ago
Read 2 more answers
If you add a solution of NaOH to a solution of H₂CO₃, two reactions occur, one after the other. Write the chemical equations for
Crazy boy [7]

We have a solution of NaOH and H₂CO₃

First, NaOH will dissociate into Na⁺ and OH⁻ ions

The Na⁺ ion will substitute one of the Hydrogen atoms on H₂CO₃ to form NaHCO₃

The H⁺ released from the substitution will bond with the OH⁻ ion to form a water molecule

If there were to be another NaOH molecule, a similar substitution will take place, substituting the second hydrogen from H₂CO₃ as well to form Na₂CO₃

6 0
2 years ago
You make a solution by putting 45.6g of iron lll carbonate into 167ml of water. What is it's molarity?
ludmilkaskok [199]
1. The molar mass of Fe2(CO3)3 is 291.72 g/mol. This means that 45.6 g is equivalent to 0.156 mol. Dividing by the 0.167 L of water gives a solution of 0.936 M.
2. Multiplying (0.672 M)(0.025 L) = 0.0168 mol. The molar mass of Ni(OH)2 is 92.71 g/mol, so multiplying by 0.0168 mol = 1.56 grams. Therefore you would need to dissolved 1.56 g of Ni(OH)2 into 25 mL of water.
3. Fe2(CO3)3 + Ni(OH)2 --> Fe(OH)3 + NiCO3Balancing: Fe2(CO3)3 + 3Ni(OH)2 --> 2Fe(OH)3 + 3NiCO3The reaction quotient is:[Fe(OH)3]^2 * [NiCO3]^3 / [Fe2(CO3)3][Ni(OH)2]^3= (0.05)^2 * (1.45)^3 / (0.936)(0.672)^3= 0.0268Since this is < 1, it implies that the reactants are favored at equilibrium.
4 0
3 years ago
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