All categories

3 years ago

HELP!!! can anyone tell me if this virtual titration lab is right & help me find the missing concentrations ??

Chemistry

2 answers:

kow [346]3 years ago

6 0

The equation that you need to use is M₁V₁=M₂V₂ for both cases since the molar ratio is 1.

In titration 1:
You would use the equation M₂=M₁V₁/V₂

M₁=concentration of NaOH (0.1M)
V₁=volume of NaOH added (16mL)
V₂=volume of HCl in the Erlenmeyer flask (20mL)
M₂=concentration of HCl in the Erlenmeyer flask (unknown)

M₂=(0.1M*16mL)/20mL
M₂=0.08M
The concentration of acid was 0.08M

Titration 2:
Still use the formula M₂=M₁V₁/V₂

M₁=concentration of HCL (0.1M)
V₁=volume of HCl added (14mL)
V₂=volume of NaOH in Erlenmeyer flask (20mL)
M₂=concentration of NaOH in the Erlenmeyer flask (unknown)

M₂=(0.1M*14mL)/20mL
M₂=0.07M
concentration of the NaOH is 0.07M

I hope this helps. Let me know if you have any further questions or if anything needs to be clarified.

malfutka [58]3 years ago

3 0

Concentration is wrong, conc=moles/volume, both concentration are wrong use the formula to correct it.

You might be interested in

How many moles of O2 are required to react completely with 1.396 g of Fe?

Gelneren [198K]

Answer:

moles O₂ needed = 0.19 mole

Explanation:

4Fe(s) + 3O₂(g) => 2Fe₂O₃(s)

1.396g Fe(s) = 1.396g/56g/mol = 0.025 mole Fe(s)

0.025 mole Fe(s) reacts with 3/4(0.025 mole O₂(g) = 0.019 mole O₂(g)

5 0

3 years ago

Which of the following is NOT a property of ionic compounds

jonny [76]

Answer:

c.Elements in the compound shares electrons

Explanation:

Because in ionic compounds element lose or gain electrons only

Sharing of electrons is the property of covlant compounds.

4 0

3 years ago

What mass of TiCl4 must react with an excess of water to produce 50.0g of TiO2 if the reaction has a 78.9% yield

Kipish [7]

Answer:

\large \boxed{\text{150 g TiCl}_{4}}

Explanation:

We will need a balanced chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ: 189.68 79.87

TiCl₄ + 2H₂O ⟶ TiO₂ + 4HCl

m/g: 50.0

To solve this stoichiometry problem, you must

Convert the actual yield to the theoretical yield
Use the molar mass of TiO₂ to convert the theoretical yield of TiO₂ to moles of TiO₂
Use the molar ratio to convert moles of TiO₂ to moles of TiCl₄
Use the molar mass of TiCl₄ to convert moles of TiCl₄ to mass of TiCt₄

1. Theoretical yield of TiO₂

$\text{Theoretical yield} = \text{50.0 g actual} \times \dfrac{\text{100 g theoretical}}{\text{78.9 g actual}} = \text{63.37 g theoretical}$

2. Moles of TiO₂

$\text{Mass of TiO}_{2} = \text{63.37 g TiO}_{2} \times \dfrac{\text{1 mol TiO}_{2}}{\text{79.87 g TiO}_{2} } = \text{0.7934 mol TiO}_{2}$

3, Moles of TiCl₄

The molar ratio is 1 mol TiO₂:1 mol TiCl₄.

$\text{Moles of TiCl}_{4} = \text{0.7934 mol TiO}_{2} \times \dfrac{\text{1 mol TiCl}_{4}}{\text{1 mol TiO}_{2}} = \text{0.7934 mol TiCl}_{4}$

4. Mass of TiCl₄

$\text{Mass of TiCl}_{4} = \text{0.7934 mol TiCl}_{4} \times \dfrac{\text{189.98 g TiCl}_{4}}{\text{1 mol TiCl}_{4}} =\textbf{150 g TiCl}_{\mathbf{4}} \\\\\text{You must use $\large \boxed{\textbf{150 g TiCl}_{\mathbf{4}}}$}$

5 0

3 years ago

A 10 pound block of lead-210 has a half-life of 22 years. What percentage of the block still contains lead-210 after 60 years?

avanturin [10]

Answer:

The percentage of the block contains 15% after 60 years.

Explanation:

Step 1: Formula for half-life time

To calculate the half-life time we will use the following formula:

At = A0 * 1/2 ^(x/t)

With At = the quantity after a time t

A0 = The quantity at time t = 0 (start)

x = time in this case = 60 years

t= half-life time = 22 years

Step 2: Calculate the percentage after 60 years

In this case: after 60 years the percentage will be

A0= 10 * 1/2 ^(60/22)

A0 = 1.5

A0 / At = 1.5 /10 = 0.15

0.15 *100% = 15 %

The percentage of the block contains 15% after 60 years.

7 0

3 years ago

Does glycine conduct electricity?<br>Does dextrose conduct electricity?

Zigmanuir [339]

Glycine: Yes.

Dextrose: No.

Hope this helps! (:

8 0

3 years ago