Which two terms represent types of chemical formulas?

Which term is used to describe the attraction that an oxygen atom has for the electrons in a chemical bond?

Mekhanik [1.2K]

electronegativty

It is the attraction force

8 0

3 years ago

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3.364 g of hydrated barium chloride of BaCL2.xH2O was dissolved in water and made up to a total volume of 250.0 mL. 10.00 mL of

atroni [7]

Given:

Mass of hydrated barium chloride = 3.364 g

Total volume of barium chloride V(total)= 250 ml

Volume taken for titration V = 10 ml

Volume of AgNO3 consumed = 46.92 ml

Concentration of AgNO3 = 0.0253 M

To determine:

The value of x i.e. the water of hydration in BaCl2

Explanation:

The net ionic equation is-

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Based on the reaction stoichiometry: Equal moles of Ag+ and Cl- combine to form AgCl

Moles of Ag+ consumed = moles of Cl- present

Moles of Ag+ = V(AgNO3) * M(AgNO3) = 0.04692 * 0.0253 = 0.00119moles

Moles of Cl- present = 0.00119 moles

Thus, 0.00119 moles of Cl- are present in 10 ml of the solution

Therefore, number of moles of Cl- in 250 ml would be-

= 0.00119 * 250 /10 = 0.02975 moles of cl-

Now:

2 moles of Cl- are present in 1 mole of BaCl2

Therefore, 0.02975 moles of Cl- correspond to- 0.02975 * 1/2 = 0.01488 moles of BaCl2

Molar mass of BaCl2 = 208.22 g/mol

Thus, mass of BaCl2 = 0.01488 moles * 208.22 g.mol-1 = 3.098 g

Mass of water of hydration = 3.364 - 3.098 = 0.266 g

# moles of water 'x' = .266/18 = 0.015 ≅ 1

Ans: Formula for hydrated barium chloride = BaCl2. 1H2O

7 0

4 years ago

HELP ME WITH MY WORK BEFORE 4:00 PLZZZZZZZZZZZZZZZZZ PEOPLEZ

Alex787 [66]

Answer:

there are 2 atoms

B) 2

Explanation:

hydrogen and one atom of oxygen bonded together.

8 0

3 years ago

If sodium sulfate was added to the mixture containing silver ions and the yellow precipitate, what might be observed after a sig

anastassius [24]

Explanation:

Very little to no formation of silver sulfate, as the silver sulfate Ksp( solubility product) is very large compared to the yellow precipitate Ksp.

By adding sodium sulfate to the silver / yellow precipitate mix, this question asks us to find a potential result and justification for the outcome. This implies that we will have to select the right answer that has a valid result and an adequate explanation for it. A substance's Ksp, or solubility product, is defined as the product of the dissolved ion concentration of each substance elevated to the power of its stoichiometric coefficient.

8 0

3 years ago

What is the molar concentration of H2SO4 in a solution made by reacting 188.9 mL of 2.086 M H2SO4 with 269.3 mL of 0.4607 M NaOH

MrRissso [65]

Answer:

0.7246 M

Explanation:

Considering:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

Or,

$Moles =Molarity \times {Volume\ of\ the\ solution}$

Given :

For $H_2SO_4$ :

Molarity = 2.086 M

Volume = 188.9 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 188.9×10⁻³ L

Thus, moles of $H_2SO_4$ :

$Moles=2.086 \times {188.9\times 10^{-3}}\ moles$

Moles of $H_2SO_4$ = 0.39405 moles

For NaOH :

Molarity = 0.4607 M

Volume = 269.3 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 269.3×10⁻³ L

Thus, moles of NaOH :

$Moles=0.4607 \times {269.3\times 10^{-3}}\ moles$

Moles of NaOH = 0.1241 moles

According to the given reaction:

$H_2SO_4_{(aq)}+2NaOH_{(aq)}\rightarrow Na_2SO_4_{(aq)}+2H_2O_{(aq)}$

1 moles of $H_2SO_4$ react with 2 moles of NaOH to form 1 mole of sodium sulfate.

Thus,

2 moles of NaOH react with 1 mole of $H_2SO_4$

1 mole of NaOH react with 1/2 mole of $H_2SO_4$

0.1241 moles of NaOH react with (1/2)×0.1241 mole of $H_2SO_4$

Moles of $H_2SO_4$ that got reacted = 0.06205 moles

Unreacted moles = Total moles - Moles that got reacted = 0.39405 - 0.06205 moles = 0.332 moles

Total volume = 188.9×10⁻³ L + 269.3×10⁻³ L = 458.2×10⁻³ L

Concentration of $H_2SO_4$ :

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity_{H_2SO_4}=\frac{0.332}{458.2\times 10^{-3}}$

Concentration of $H_2SO_4$ = 0.7246 M

5 0

4 years ago