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KiRa [710]
3 years ago
7

Predict whether or not a precipitate forms upon mixing 175.0 ml of a 0.0055 mkcl solution with 145.0 ml of a 0.0015 m agno3 solu

tion. identify the precipitate, if any. express your answer as a chemical formula. enter noreaction if no precipitate is formed.
Chemistry
1 answer:
REY [17]3 years ago
8 0

Step 1: Write down the chemical reaction

KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)

The precipitate that can be expected is AgCl

Step 2: Calculate the moles of KCl and AgNO3

# moles of KCl = V(KCl) * M(KCl)

                        = 0.175 L * 0.0055 moles/L = 9.63*10⁻⁴ moles

# moles of AgNO3 = V(AgNO3) * M(AgNO3)

                        = 0.145 L * 0.0015 moles/L = 2.18*10⁻⁴ moles

Since moles of AgNO3 < KCl, the former is the limiting reagent

Therefore, moles of AgCl formed = 2.18*10⁻⁴ moles

Step 3: Predict if AgCl precipitate will be formed

The solubility product Ksp for AgCl = 1.6 *10⁻¹⁰

i.e.

AgCl(s) ↔ Ag⁺(aq) + Cl⁻(aq)

Ksp = [Ag+][Cl-]

if [Ag+][Cl-] > Ksp then precipitation will occur

Now total volume of the solution = 175 + 145 = 320 ml = 0.320 L

[Ag+] = [Cl-] = 2.18*10⁻⁴ moles/0.320 L = 6.81*10⁻⁴ M

[Ag+][Cl-] = (6.81*10⁻⁴)² = 4.64 *10⁻⁷

Since  [Ag+][Cl-] > Ksp, AgCl precipitate will be formed.


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ss7ja [257]

Answer:

Light as a wave: Light can be described (modeled) as an electromagnetic wave. In this model, a changing electric field creates a changing magnetic field. This changing magnetic field then creates a changing electric field and BOOM - you have light. ... So, Maxwell's equations do say that light is a wave.

Explanation:

Hope this helps

6 0
3 years ago
Read 2 more answers
A 1.68 g sample of water is injected into a closed evacuated 5.3 liter flask at 65°C. What percent (by mass) of the water will b
Angelina_Jolie [31]

Answer:

50.4 % of the water will be vapor

Explanation:

<u>Step 1:</u> Data given

Mass of water = 1.68 grams

volume of the flask = 5.3 L

Temperature = 65°C

Vapor pressure of water at 65°C = 187.5 mmHg = 0.2467 atm

<u>Step 2:</u> Calculate moles of H2O

p*V=n*R*T

⇒ p = the pressure of water = 0.2467 atm

⇒ V = the volume of the flask = 5.3 L

⇒ n = moles of water

⇒ R = gas constant = 0.08206 L*atm/ K*mol

⇒ T = the temperature = 65°C = 338 Kelvin

n = (p*V)/(R*T)

n = (0.2467 * 5.3) /(0.08206* 338)

n = 0.047 moles

<u>Step 3:</u> Calculate mass of water

Mass of water = moles of water * molar mass of water

Mass of water = 0.047 moles *18.02 g/mol

Mass of water = 0.84694 grams

<u>Step 4:</u> Calculate the percent of water vaporized

% = (0.84694 grams/1.68 grams) *100%

% = 50.4%

50.4 % of the water will be vapor

5 0
3 years ago
SHOW YOUR WORK!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
WARRIOR [948]

Answer:

1.375%

Explanation:

Percent Error = measured value - accepted value/ accepted value x 100

Measured Value: 15.78

Accepted Value: 16.00

Work:

\frac{15.78-16.00}{16.00} * 100

\frac{-.22}{16} * 100 = -1.375

You cannot have a negative percentage. Therefore the answer is 1.375%

4 0
3 years ago
a fixed amount of gas at 25.0 degrees Celsius occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles law to calc
kirill [66]

Explanation:

Since pressure remained constant, we can eliminate P from the equation

\frac{pv }{t}  =  \frac{pv}{t}

Doing some algebra and converting temperature to Kevin by adding 273, you should obtain the same result.

8 0
3 years ago
if a standard die is rolled twice what is the probability of getting a perfect square,then a number that is less than 5.
solniwko [45]
There are three perfect squares in a standard die; 1, 2, 4. If there is two standard dies, then the probability of getting a perfect square is 1/3 x 1/3 = 1/9. 
There are 4 numbers less than 5 in a standard die, making it 1/4 x 1/4=1/16. 
5 0
3 years ago
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