CHEMISTRY COLLEGE

Vinegar, the commercial name for acetic acid, HC2Hs02, is a monoprotic organic acid. A 5% (w/v) solution of vinegar is used to titrate a sample of an antacid that contains CaCO3 is the only basic component. If one antacid tablet contains 800 mg of CaCOs in it, then calculate how many milliliters of vinegar should be required to completely neutralize the CaCO3 present in one tablet of antacid?

Answers

Answer 1

Answer:

19.2 g of vinegar solution

Explanation:

Here we have the chemical reaction between acetic acid (CH₃COOH) and calcium carbonate (CaCO₃):

2 CH₃COOH + CaCO₃ → (CH₃COO)₂Ca + CO₂ + H₂O

number of moles = mass / molecular weight

number of moles of CaCO₃ = 0.8 / 100 = 0.008 moles

Knowing the chemical reaction, we devise the following reasoning:

if 2 moles of CH₃COOH react with 1 moles of CaCO₃

then X moles of CH₃COOH react with 0.008 moles of CaCO₃

X = (2 × 0.008) / 1 = 0.016 moles of CH₃COOH

mass = number of moles × molecular weight

mass of acetic acid (CH₃COOH) = 0.016 × 60 = 0.96 g

Now to find the volume of vinegar acid (solution of acetic acid) with a concentration of 5% (weight/volume) we use the following reasoning:

if there are 5 g of acetic acid in 100 mL of vinegar solution

then there are 0.96 g of acetic acid in Y mL of vinegar solution

Y = (0.96 × 100) / 5 = 19.2 g of vinegar solution

Learn more about:

weight/volume concentration

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Answers

Answer:

a. false

b. true

c. false

d. false

e. false

f. false

Q2: Both have electrons orbiting around the nucleus; Bohr's model is more detailed and expands on Rutherford's

Q5:

Ne = neon

Al = aluminum

K = potassium

Ne = 10 electrons/protons

Al = 13 electrons/protons

K = 19 electrons/protons

Consider two aqueous solutions of NaCl. Solution 1 is 4.00 M and solution 2 is 0.10 M. In what ratio (solution 1 to solution 2) must these solutions be mixed in order to produce a 0.86 M solution of NaCl

Answers

Answer:

The ratio of solution 1 to solution 2 is 24.20 to 100.00.

Explanation:

We will mix V₁ (L) of solution 1 with V₂ (L) of solution 2 to get the final solution.

So the mole concentration in the final solution is calculated as below, note that C₁ is the concentration of solution 1, and C₂ is the concentration of solution 2

$[M] = (V_(1) C_(1) +V_(2)C_(2))/(V_(1)+V_(2)) = \frac{4 V_(1) + 0.1 V_(2)}_{V_(1)+V_(2)}}=0.86$

Then we can calculate for the ratio

$(V_(1))/(V_(2))=(0.86-0.10)/(4.00-0.86) =(0.76)/(3.14)$ or $(24.20)/(100.00)$

What will be the theoretical yield of tungsten(is) ,W, if 45.0 g of WO3 combines as completely as possible with 1.50 g of H2

Answers

Answer:

35.6 g of W, is the theoretical yield

Explanation:

This is the reaction

WO₃ + 3H₂ → 3H₂O + W

Let's determine the limiting reactant:

Mass / molar mass = moles

45 g / 231.84 g/mol = 0.194 moles

1.50 g / 2 g/mol = 0.75 moles

Ratio is 1:3. 1 mol of tungsten(VI) oxide needs 3 moles of hydrogen to react.

Let's make rules of three:

1 mol of tungsten(VI) oxide needs 3 moles of H₂

Then 0.194 moles of tungsten(VI) oxide would need (0.194 .3) /1 = 0.582 moles (I have 0.75 moles of H₂, so the H₂ is my excess.. Then, the limiting is the tungsten(VI) oxide)

3 moles of H₂ need 1 mol of WO₃ to react

0.75 moles of H₂ would need (0.75 . 1)/3 = 0.25 moles

It's ok. I do not have enough WO₃.

Finally, the ratio is 1:1 (WO₃ - W), so 0.194 moles of WO₃ will produce the same amount of W.

Let's convert the moles to mass (molar mass . mol)

0.194 mol . 183.84 g/mol = 35.6 g

In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)

Answers

It is called, Noble gas

When palmitoleic acid reacts with hydrogen to form a saturated fatty acid, indicate the stoichiometry of the reaction and the product that is formed. If the stoichiometry of H2 or the product is not integral, enter a fraction (i.e. 3/2)

Answers

Answer:

Stoichiometric coefficient of hydrogen gas is 1.

Stoichiometric coefficient of palmitic acid is 1.

Explanation:

Addition of hydrogen to double bond is termed as hydrogenation reaction.

$C_(16)H_(30)O_2+H_2\rightarrow C_(16)H_(32)O_2$

According to stoichiometry, 1 mole of palmitoleic acid reacts with 1 mole of hydrogen gas to give 1 mole of palmitic acid.

Stoichiometric coefficient of hydrogen gas is 1.

Stoichiometric coefficient of palmitic acid is 1.

A student who is performing this experiment pours an 8.50 mL sample of the saturated borax solution into a 10 mL graduated cylinder after the borax solution had cooled to a certain temperature T. The student rinses the sample into a small beaker using distilled water, and then titrates the solution with a 0.500 M HCl solution. 12.00 mL of the HCl solution is needed to reach the endpoint of the titration.Calculate the value of Ksp for borax at temperature T.