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3 years ago

How do I see answer to question already asked by someone else that I need immediately?!

Chemistry

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Alecsey [184]3 years ago

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Enter the balanced complete ionic equation for HCl(aq)+K2CO3(aq)→H2O(l)+CO2(g)+KCl(aq). Express your answer as a chemical equati

Marat540 [252]

<u>Answer:</u> The net ionic equation is given below.

<u>Explanation:</u>

Net ionic equation of any reaction does not include any spectator ions.

These ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form.

The chemical equation for the reaction of hydrochloric acid and potassium carbonate is given as:

$2HCl(aq.)+K_2CO_3(aq.)\rightarrow H_2O(l)+CO_2(g)+2KCl(aq.)$

Ionic form of the above equation follows:

$2H^+(aq.)+2Cl^-(aq.)+2K^+(aq.)+CO_3^{2-}(aq.)\rightarrow CO_2(g)+H_2O(l)+2K^+(aq.)+2Cl^-(aq.)$

As, potassium and chloride ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation.

The net ionic equation for the above reaction follows:

$2H^+(aq.)+CO_3^{2-}(aq.)\rightarrow CO_2(g)+H_2O(l)$

Hence, the net ionic equation is given above.

7 0

3 years ago

How many grams are in 4.5 x 10^22 molecules of water? please show dimensional analysis

GaryK [48]

Answer:

1.1grams

Explanation:

Find moles of water:

4.5x10^22/(6.02x10^23)=0.07mol

Find molar mass of the water

O=16.00g/mol

0.07x 16.00=1.1 grams

4 0

3 years ago

alculate the pH of the solution, upon addition of 0.035 mol of NaOH to the original buffer. Express your answer using two decima

svetlana [45]

A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.

Calculate the pH of the solution, upon addition of 0.035 mol of NaOH to the original buffer.

Answer:

The pH of this solution = 5.06

Explanation:

Given that:

number of moles of CH3COOH = 0.100 mol

volume of the buffer solution = 1.0 L

number of moles of NaC2H3O2 = 0.100 mol

The objective is to Calculate the pH of the solution, upon addition of 0.035 mol of NaOH to the original buffer.

we know that concentration in mole = Molarity/volume

Then concentration of [CH3COOH] = $\mathtt{ \dfrac{0.100 \ mol}{ 1.0 \ L }}$ = 0.10 M

The chemical equation for this reaction is :

$\mathtt{CH_3COOH + OH^- \to CH_3COO^- + H_2O}$

The conjugate base is CH3COO⁻

The concentration of the conjugate base [CH3COO⁻] is = $\mathtt{ \dfrac{0.100 \ mol}{ 1.0 \ L }}$

= 0.10 M

where the pka (acid dissociation constant)for CH3COOH = 4.74

If 0.035 mol of NaOH is added to the original buffer, the concentration of NaOH added will be = $\mathtt{ \dfrac{0.035 \ mol}{ 1.0 \ L }}$ = 0.035 M

The ICE Table for the above reaction can be constructed as follows:

$\mathtt{CH_3COOH \ \ \ + \ \ \ \ OH^- \ \ \to \ \ CH_3COO^- \ \ \ + \ \ \ H_2O}$

Initial 0.10 0.035 0.10 -

Change -0.035 -0.035 + 0.035 -

Equilibrium 0.065 0 0.135 -

By using Henderson-Hasselbalch equation:

The pH of this solution = pKa + log $\mathtt{\dfrac{CH_3COO^-}{CH_3COOH}}$

The pH of this solution = 4.74 + log $\mathtt{\dfrac{0.135}{0.065}}$

The pH of this solution = 4.74 + log (2.076923077 )

The pH of this solution = 4.74 + 0.3174

The pH of this solution = 5.0574

The pH of this solution = 5.06 to two decimal places

7 0

3 years ago

The temperature of gas is 100 K and its volume is 500 ml. If the volume is increased to 1000.0 ml, what is the new temperature o

Mashutka [201]

Answer:

my digc fell off your mom pu___ssy

Explanation:

;o is ajoke

6 0

3 years ago

What could cause a build up of algae which would decrease the amount of oxygen available for the organisms in the river? protect

miv72 [106K]

Answer:

In addition, other pollutants like fertilizers, pesticides, and heavy metals are often attached to the soil particles and wash into the water bodies, causing algal blooms and depleted oxygen, which is deadly to most aquatic life.

7 0

3 years ago