What is the molality of a solution

Answers

Answer 1

Answer:

Answer:

The formula for molality is m = moles of solute / kilograms of solvent. In problem solving involving molality, we sometimes need to use additional formulas to get to the final answer. One formula we need to be aware of is the formula for density, which is d = m / v, where d is density, m is mass and v is volume

Explanation:

it is a measure of the concentration of a solute in a solution in terms of amount of substance in a specified amount of mass of the solvent. This contrasts with the definition of molarity which is based on a specified volume of solution.

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The maximum energy available for useful work from a spontaneous reaction(A) free energy
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Answers

The answer is: A; Free Energy

What is the van't hoff factor of C7H7NO?

Answers

Answer:

i = 1

Explanation:

Van't Hoff factor (i) is explained as the number of ions dissolved in solution.

It is needed to determine colligative properties which depend on the amount of solute.

C₇H₇NO is an organic compound → benzamide

All the organic compound have 1, as Van't Hoff factor.

In order to predict i, you consider ionic salts. For example:

AlCl₃

CaCl₂

NH₄NO₃

When you dissociate them, you determine i:

AlCl₃ → Al³⁺ + 3Cl⁻ i =4

CaCl₂ → Ca²⁺ + 2Cl⁻ i = 3

NH₄NO₃ → NH₄⁺ + NO₃⁻ i =2

12. A salt used as a fertiliser has the empirical formula H4N2O3.Suggest the formulae of the ions present in this salt

Answers

Final answer:

The formula H4N2O3 represents a salt containing ammonium (NH4+) and nitrate (NO3-) ions. These ions are often present in fertilisers because they effectively deliver nitrogen to plants.

Explanation:

The empirical formula H4N2O3 represents a salt used in fertilisers and it contains hydrogen, nitrogen, and oxygen. In this salt, the ions present are the ammonium ion (NH4+) and the nitrate ion (NO3-). Hydronium and nitrogen dioxide might also be present in the compound. However, the most relevant ions are generally the ammonium and the nitrate ions, because they are often used in fertilizers due to their abilities to effectively deliver nitrogen to plants.

Learn more about Chemical ions here:

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The empirical formula H4N2O3 suggests that in this salt, there are two nitrogen (N) atoms, three oxygen (O) atoms, and four hydrogen (H) atoms. To determine the formulae of the ions present, we can consider that hydrogen usually forms H+ ions, while nitrogen can form N3- ions, and oxygen can form O2- ions.

Based on this, the formulae of the ions present in this salt could be:

- Cation: H+
- Anions: N3- and O2-

So, the salt might consist of H+ cations and a combination of N3- and O2- anions, depending on the specific compound.

What volume do 4.96 moles of O2 occupy at STP?

Answers

Answer: Step 1: List the known quantities and plan the problem. Known. 4.96 moles O2; 1 mol = 22.4

Explanation: I hope that helped.

Suppose the mole number of Ca2+ ions in a 50 mL water sample is quantified as 1.5 × 10−5 mol. What is the concentration of Ca2+ ions in the water sample in ppm CaCO3?

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$(1.5x 10^(-5) mol Ca^(2+))/(50ml) ( (1 mol CaC O_(3) )/(1 mol Ca^(2+) ) )( (100,000 ppm)/(1 molCaC O_(3)/L ) ) \n =0.0300234$

Answer : The concentration of $Ca^(2+)$ ions in the water sample in ppm is, 12000 ppm

Solution : Given,

Moles of calcium = $1.5* 10^(-5)moles$

Molar mass of calcium = 40 g/mole

Volume of solution = 50 ml

First we have to calculate the mass of calcium.

$\text{Mass of calcium}=\text{Moles of calcium}* \text{Molar mass of calcium}=(1.5* 10^(-5)moles)* (40g/mole)=60* 10^(-5)g=6000mg$

(1 g = 1000 mg)

Now we have to calculate the concentration of calcium.

$\text{Concentration of calcium}=\frac{\text{Mass of calcium}* 1000}{\text{Volume of solution}}=(6000mg* 1000)/(50ml)=12000mg/L=12000ppm$

(1 ppm = 1 mg/L)

Therefore, the concentration of $Ca^(2+)$ ions in the water sample in ppm is, 12000 ppm

What is first ionization energy

Answers

Hope this helps...Definition. The first ionisation energy is the energyrequired to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+.

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