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konstantin123 [22]
3 years ago
15

What is the concentration of nitrate ions in a 0.225 msr(no3)2 solution?

Chemistry
2 answers:
12345 [234]3 years ago
7 0

Answer : The concentration of nitrate ions is 0.450 m.

Solution : Given,

Molarity of Sr(NO_3)_2 = 0.225 m

The balanced ionic equation is,

Sr(NO_3)_2\rightarrow Sr^{+2}+2NO^-_3

From the reaction, we conclude that the 1 mole of Sr(NO_3)_2 produces 2 moles of NO^-_3 ions. That means the concentration of nitrate ions is twice the value of Sr(NO_3)_2.

then, 0.225 m of Sr(NO_3)_2 gives 2 × 0.225 of NO^-_3 ions

Now the concentration of NO^-_3 ions is equal to 0.450 m.


BabaBlast [244]3 years ago
5 0

We are given that there are 2 moles of NO3 from the 0.225 M Sr(NO3)2 solution. Therefore we simply use stoichiometry to solve this problem.

 

Concentration NO3 = 0.225 M Sr(NO3)2 * (2 moles NO3 / 1 mole Sr(NO3)2)

<span>Concentration NO3 = 0.45 M</span>

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A 1 liter solution contains 0.247 M nitrous acid and 0.329 M sodium nitrite. Addition of 0.271 moles of calcium hydroxide will:
Inessa05 [86]

Answer:

a. Raise the pH slightly

Explanation:

We know that

Pka of HNO2/KNO2 =3.39

Moles of HNO2 in the buffer=0.247 mol/L×1L=0.247 moles

Moles of NO2-=0.329mol/L×1L=0.329 moles

If 0.271 moles of Ca(OH)2 is added it will neutralise 0.136 moles of acid ,HNO2,remaining HNO2=0.247-0.136=0.111 moles

Moles of NO2- will increase as 0.0333 moles Ca(NO)2 will be formed =0.0333+0.036=0.0693 moles

pH=pka+log [base]/[acid]      {henderson -hasselbach equation}

=3.39+log (0.0693/0.0317)=3.39+0.34=3.73

pH=3.73

4 0
4 years ago
Calculate the molar solubility of silver(i) bromate with ksp = 5. 5×10-5. also, convert the molar solubility to the solubility.
Sindrei [870]

The molar solubility is 7.4×10^{-3} M and the solubility is  7.4×10^{-3} g/L .

Calculation ,

The dissociation of silver bromide is given as ,

AgBr → Ag ^{+} + Br^{-}

S  

 -          S        S        

Ksp =  [Ag ^{+} ] [ Br^{-} ]  =  [S] [ S ] = S^{2}

S = √ Ksp = √ 5. 5×10^{-5} = 7.4×10^{-3}

The solubility =7.4×10^{-3} g/L

The molar solubility is the solubility of one mole of the substance.

Since ,  one mole of AgBr is dissociates and form one mole of each  Ag ^{+} and Br^{-} ion . So, solubility is equal to molar solubility but unit is different.

Molar solubility = 7.4×10^{-3} mol/L = 7.4×10^{-3} M

To learn more about molar solubility ,

brainly.com/question/16243859

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7 0
1 year ago
What happens in nuclear fission reactions?
Dmitry [639]

Answer:

in nuclear fission, an unstable atom splits into 2 or more smaller pieces that are more stable and releases energy in the process. the fission process also releases extra neutrons which can split additional atoms, resulting in a chain reaction that releases a lot of energy

8 0
3 years ago
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How is a radioactive element different from a stable element?
USPshnik [31]
A radioactive element has an unstable nucleus that emits particles in the form of alpha, beta, or gamma radiation. A stable element has a nucleus that does not emit such particles
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3 years ago
Calculate the pH of a solution prepared by mixing: (Show your work for these calculations) pk of acetic acid is 4.75 a. two mole
kupik [55]

Answer:

Explanation:

To calculate pH you need to use Henderson-Hasselbalch formula:

pH = pka + log₁₀ \frac{[A^-]}{[HA]}

Where HA is the acid concentration and A⁻ is the conjugate base concentration.

The equilibrium of acetic acid is:

CH₃COOH ⇄ CH₃COO⁻ + H⁺ pka: 4,75

Where <em>CH₃COOH </em>is the acid and <em>CH₃COO⁻ </em>is the conjugate base.

Thus, Henderson-Hasselbalch formula for acetic acid equilibrium is:

pH = 4,75 + log₁₀ \frac{[CH_{3}COO^-]}{[CH_{3}COOH]}

a) The pH is:

pH = 4,75 + log₁₀ \frac{[2 mol]}{[2 mol]}

<em>pH = 4,75</em>

<em></em>

b) The pH is:

pH = 4,75 + log₁₀ \frac{[2 mol]}{[1mol]}

<em>pH = 5,05</em>

<em></em>

I hope it helps!

7 0
4 years ago
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