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vagabundo [1.1K]
2 years ago
5

What is the empirical formula and empirical formula mass for the following compound? C3H6O3?

Chemistry
1 answer:
babunello [35]2 years ago
5 0
Answer: C3H6O3 > CH2O
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Determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide.
a_sh-v [17]

The volume of H₃PO₄ : 13.33 ml

<h3>Further explanation</h3>

Given

0.003 M  Phosphoric acid-H₃PO₄

40 ml of 0.00150 M Calcium hydroxide-Ca(OH)₂

Required

Volume of H₃PO₄

Solution

Acid-base titration formula  

Ma. Va. na = Mb. Vb. nb  

Ma, Mb = acid base concentration  

Va, Vb = acid base volume  

na, nb = acid base valence  (amount of H⁺/OH⁻)

H₃PO₄⇒3H⁺ + PO₄³⁻ ⇒ 3 H⁺ = valence = 3

Ca(OH)₂⇒Ca²⁺ + 2OH⁻⇒ 2 OH⁻ = valence = 2

Input the value :

a = H₃PO₄, b = Ca(OH)₂

0.003 x Va x 3 = 0.0015 x 40 x 2

Va = 13.33 ml

8 0
2 years ago
The density of mercury is 13.5g/mL. What is the volume of this liquid if the sample weighs 12.5 pounds?
Mama L [17]

Answer : The volume of liquid is 420 mL.

Explanation :

Density : The mass per unit volume of a substance is known as density.

Formula used:

\text{Density}=\frac{\text{Mass}}{\text{Volume}}

As we are given:

Density of mercury = 13.5 g/mL

Mass = 12.5 pounds

First we have to convert mass of sample from pound to gram.

Conversion used:

As, 1 pound = 453.6 g

So, 12.5 pounds = 453.6 × 12.5 g = 5670 g

Now we have to calculate the volume of liquid.

\text{Density}=\frac{\text{Mass}}{\text{Volume}}

Now putting all the given values in this formula, we get:

13.5g/mL=\frac{5670g}{\text{Volume}}

Volume = 420 mL

Therefore, the volume of liquid is 420 mL.

7 0
3 years ago
Please help ASAP I will give Brainliest
MaRussiya [10]

Answer:

17.6 grams of nitrogen gas

4 0
3 years ago
to form brass, copper and zinc combine but do not chemically bond. brass is a(n) ________. a atom b element c compound d
umka21 [38]

Answer: Mixture

Explanation:To form brass, copper and zinc combine but do not chemically bond. Brass is a(n)

3 0
2 years ago
An unknown triprotic acid (H3A) is titrated with NaOH. After the titration Ka1 is determined to be 0.0013 and Ka2 is determined
e-lub [12.9K]

Answer:

6.68 X 10^-11

Explanation:

From the second Ka, you can calculate pKa = -log (Ka2) = 6.187

The pH at the second equivalence point (8.181) will be the average of pKa2  and pKa3. So,

8.181 = (6.187 + pKa3) / 2

Solving gives pKa3 = 10.175, and Ka3 = 10^-pKa3 = 6.68 X 10^-11

7 0
3 years ago
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