When liquid phosphorus trichloride is added to water, it reacts to form aqueous phosphorous acid, h3po3(aq), and aqueous hydrochloric acid. express your answer as a balanced chemical equation. identify all of the phases in your answer?

Answers

Answer 1

Answer:

Answer: The balanced chemical equation for the reaction of phosphorus trichloride with water is written below.

Explanation:

A balanced chemical equation is defined as the equation in which total number of individual atoms on the reactant side is equal to the total number of individual atoms on product side.

The balanced chemical equation for the reaction of phosphorus trichloride with water follows:

$PCl_3(l)+3H_2O(l)\rightarrow H_3PO_3(aq.)+3HCl(aq.)$

By Stoichiometry of the reaction:

1 mole of liquid phosphorus trichloride reacts with 3 moles of water to produce 1 mole of aqueous phosphorus acid and 3 moles of aqueous hydrochloric acid.

Hence, the balanced chemical equation for the reaction of phosphorus trichloride with water is written above.

Answer 2

Answer:

Hey there!:

I'll balance it:

PCl3 + H2O ---> H3PO3 + HCl

* PCl3 (l )+ 3 H2O (l)--->H3PO3(aq) +3 HCl(aq)

Hope that helps!

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Perform the calculation and report the answer using the proper number of significant figures. Make sure the answer is rounded correctly. 1.012×10^-3 J/(0.015456 g)(298.3682−298.3567)K

Answers

Answer:

$=5.694(J)/(g*K)$

Explanation:

Hello,

In this case, since the result of the operation between two magnitudes is shown with the same significant figures of the shortest number, we obtain:

$1.012x10^(-3) J/[(0.015456 g)(298.3682-298.3567)]K$

Next, we proceed as follows:

$=0.065476J/[(g)(20.0115K)]\n\n=5.693582(J)/(g*K)$

Nevertheless, since 1.012 is the shortest number and has four significant figures, the result is rounded to four significant figures, that is until the three but it rounded due to the fact that the next digit is five:

$=5.694(J)/(g*K)$

Regards.

Which description is not a property of a base? (2 points)a
pH lower than 7

b
Turns litmus paper blue

c
Bitter taste

d
Slimy feel

Answers

i think it’s A
because if the pH is lower than 7 than it is acidic

Answer:

the answer is a hope it helps.

Explanation:

How many moles of argon are in 4.80x10^24 atoms of argon

Answers

Answer:

7.97 mol Ar

Explanation:

Use Avogadro's number to convert atoms to moles. This number is the number of atoms in one mole. There are 6.022 × 10²³ atoms in one mole.

Divide the number of atoms given by Avogadro's number.

(4.80 × 10²⁴)/(6.022 × 10²³) = 7.97 mol

There are 7.97 moles of argon.

Answer:

3.0 moles (A P E X)

Explanation:

What substance is produced by the reaction: H+[aq]+OH-[aq]=?

Answers

Answer:

It produces water.

Explanation:

H+ + OH- produces H2O.

It is a type of Neutralization reaction.

A 25.0mL solution acetic acid (CH3CO2H) is titrated with 0.20M NaOH and reaches the endpoint after the addition of 16.3mL of NaOH. What is the concentration of acetic acid in solution

Answers

Answer: 0.1304M

Explanation: Please see the attachments below

Final answer:

The concentration of acetic acid in the solution is 0.1304 M.

Explanation:

To determine the concentration of acetic acid in solution, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between acetic acid and sodium hydroxide. The balanced equation is:

CH3CO2H + NaOH -> CH3CO2Na + H2O

From the balanced equation, we can see that 1 mole of acetic acid reacts with 1 mole of sodium hydroxide. In order to calculate the moles of acetic acid, multiply the volume of NaOH used (16.3 mL) by the molarity of NaOH (0.20 M), then divide the result by 1000 to convert mL to L:

Moles of acetic acid = (16.3 mL NaOH x 0.20 M NaOH) / 1000 = 0.00326 moles

Now, to calculate the concentration of acetic acid in the solution, we divide the moles of acetic acid by the volume of the solution in litres:

Concentration of acetic acid = (0.00326 moles) / (25.0 mL x 1 L/1000 mL) = 0.1304 M

This means that the concentration of the acetic acid in the solution is 0.13M.

Learn more about Concentration of acetic acid here:

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