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3 years ago

Enter the ions formed when (NH4)2S dissolves in water.

Chemistry

2 answers:

lisabon 2012 [21]3 years ago

5 0

The ions formed are NH4(+) and S(2-)

The dissolution reaction of (NH4) 2S in water is as follows:

(NH4) 2S ==> 2 NH4 (+) + S (2-).

Ammonium sulfide is the ammonium salt of hydrogen sulfide. It has the formula (NH4) 2S and belongs to the sulfide family.

It is a relatively unstable compound (crystals decomposing at -18 ° C, but exists and is more stable in aqueous solution.) With a pKa exceeding 15, the hydrosulfide ion cannot be significantly deprotonated by ammonia. Thus, such solutions consist mainly of a mixture of ammonia and hydrosulphide of ammonium, it has a smell, close to that of hydrogen sulfide, and its aqueous solutions can be precisely by emitting H2S.

kirill [66]3 years ago

5 0

The ions formed are NH4+ and SO4^2-
When (NH4)2SO4 is dissolved in water, ammonium ion and a sulfate ion are produced due to the reaction between (NH4)2SO4 and water. Ions are produced when simple polar molecules are dissolved in water, the molecules dissociate into ions on dissolving it in water. Ammonium ion formed is positively charged while the sulfate ion is negatively charged.

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__H2 + __O2 --> __H2O

nekit [7.7K]

Answer:

42.3moles

Explanation:

The chemical equation given in this question is as follows:

H2 + O2 → H2O

However, this equation is unbalanced, the balanced chemical equation is as follows:

2H2 + O2 → 2H2O

This equation shows that;

2 moles of hydrogen gas (H2) will produce 2 moles of water (H2O)

Hence, If 42.3 moles of water (H2O) are produced, 42.3 × 2/2

= 42.3moles of hydrogen was reacted.

6 0

3 years ago

Determine the number of atoms and the mass of zirconium, silicon and oxygen found in 0.3384 Mol of zircon ZrSiO4, a

sattari [20]

Explanation:

1 mol of ZrSiO₄ , have , 1 mol of Zr , 1 mol of Si and 4 mol of Oxygen .

since ,

1 mol of a substance have 6.022 * 10 ²³ particles ,

From the question ,

0.3384 mol of zircon ZrSiO₄ ,

hence ,

from the above equation ,

1 mol of a substance have 6.022 * 10 ²³ particles ,

0.3384 mol = 0.3384 * 6.022 * 10 ²³ number of atoms

= 2.037 * 10 ²³ number of atoms

Hence ,

0.3384 mol of ZrSiO₄ will have , 0.3384 mol of Zr ,0.3384 mol of Si and 4*0.3384 mol of Oxygen .

Hence ,

number of atoms of Zr = 0.3384 mol * 6.022 * 10 ²³ = 2.037 * 10 ²³ number of atoms

number of atoms of Si = 0.3384 mol * 6.022 * 10 ²³ = 2.037 * 10 ²³ number of atoms

number of atoms of O = 4 * 0.3384 mol * 6.022 * 10 ²³ = 8.148 * 10 ²³ number of atoms

The mass is calculated as -

since ,

Moles is denoted by given mass divided by the molecular mass ,

Hence ,

n = w / m

n = moles ,

w = given mass ,

m = molecular mass .

n = w / m

w = n * m

mass of Zr ,

Since we know , the molecular mass of Zr = 91 g/mol

moles of Zr = 0.3384 mol

using the above formula ,

w = n * m

w = 0.3384 mol * 91 g/mol = 30.79 g

hence ,

The mass of Zr = 30.79 g

mass of Si ,

Since we know , the molecular mass of Si = 28 g/mol

moles of Si = 0.3384 mol

using the above formula ,

w = n * m

w = 0.3384 mol * 28 g/mol = 9.475 g

hence ,

The mass of Si = 9.475 g

mass of O ,

Since we know , the molecular mass of O = 16 g/mol

moles of Si = 1.3536 mol

using the above formula ,

w = n * m

w = 1.3536 mol * 16 g/mol = 21.65 g

hence ,

The mass of O = 21.65 g

8 0

3 years ago

A solution is made by dissolving 100. g of cobalt(III)chloride in 250. g of water. to make a solution that has a density of 1.25

Mariulka [41]

Answer:

Option A) (I) 2.42 m (II) 2.16 M

Explanation:

Let's determine some information.

Solute = CoCl₃ (molar mass = 165.29 g/m); mass of 100 g

Solvent = Water, mass of 250 g

Solution mass = mass of CoCl₃ + mass of water

250 g + 100 g = 350 g of solution

If we want to reach molarity (mol/L), let's determine solution volume with density:

Solution density = solution mass / solution volume

1.25 g/mL = 350 g / solution volume

Solution volume = 350 g / 1.25 g/mL = 280 mL

Let's convert the volume to L → 280 mL = 0.280L

Let's convert the mass of solute to moles = 100 g / 165.29 g/m →0.605 mol

Mol/L = 0.605 moles / 0.280 L = 2.16 M

Now let's calculate molalilty (mol/kg of solvet)

We must convert solvent mass to kg → 250g = 0.250 kg

Then, 0.605 moles / 0.250 kg =2.42 m

8 0

4 years ago

Which line of defense includes active immunity?<br><br> first<br> second<br> third<br> fourth

Tom [10]

Answer:

B second

Explanation:

4 0

3 years ago

Read 2 more answers

To what volume should you dilute 122 mL of an 8.20 M CuCl2 solution so that 51.0 mL of the diluted solution contains 4.40 g CuCl

BartSMP [9]

Answer:

<h2>The first thing to do here is to use the molarity and the volume of the initial solution to figure out how many grams of copper(II) chloride it contains.</h2><h2 /><h2>133</h2><h2>mL solution</h2><h2>⋅</h2><h2>1</h2><h2>L</h2><h2>10</h2><h2>3</h2><h2>mL</h2><h2>⋅</h2><h2>7.90 moles CuCl</h2><h2>2</h2><h2>1</h2><h2>L solution</h2><h2>=</h2><h2>1.051 moles CuCl</h2><h2>2</h2><h2 /><h2>To convert this to grams, use the compound's molar mass</h2><h2 /><h2>1.051</h2><h2>moles CuCl</h2><h2>2</h2><h2>⋅</h2><h2>134.45 g</h2><h2>1</h2><h2>mole CuCl</h2><h2>2</h2><h2>=</h2><h2>141.31 g CuCl</h2><h2>2</h2><h2 /><h2>Now, you know that the diluted solution must contain </h2><h2>4.49 g</h2><h2> of copper(II) chloride. As you know, when you dilute a solution, you increase the amount of solvent while keeping the amount of solute constant.</h2><h2 /><h2>This means that you must figure out what volume of the initial solution will contain </h2><h2>4.49 g</h2><h2> of copper(II) chloride, the solute.</h2><h2 /><h2>4.49</h2><h2>g</h2><h2>⋅</h2><h2>133 mL solution</h2><h2>141.32</h2><h2>g</h2><h2>=</h2><h2>4.23 mL solution</h2><h2>−−−−−−−−−−−−−− </h2><h2 /><h2>The answer is rounded to three sig figs.</h2><h2 /><h2>You can thus say that when you dilute </h2><h2>4.23 mL</h2><h2> of </h2><h2>7.90 M</h2><h2> copper(II) chloride solution to a total volume of </h2><h2>51.5 mL</h2><h2> , you will have a solution that contains </h2><h2>4.49 g</h2><h2> of copper(II) chloride.</h2>

3 0

3 years ago