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irinina [24]
3 years ago
13

Calculate the concentration of H3O+ in a solution that contains 5.5 × 10-5 M OH- at 25°C. Identify the solution as acidic, basic

, or neutral.
a. 1.8 × 10-10 M, acidic
b. 9.2 × 10-1 M, basic
c. 5.5 × 10-10 M, neutral
d. 9.2 × 10-1 M, acidic
e. 1.8 × 10-10 M, basic
Chemistry
1 answer:
defon3 years ago
6 0

Answer:

The correct answer is option (e).

Explanation:

Concentration of hydroxide ions [OH^-]= 5.5\times 10^{-5} M

The pOH of the solution is defined as negative logarithm of hydroxide ions of in an aqueous solution.

  • Higher the value of pOH more will be the acidic solution.
  • Lower the value of pOH more will be the basic solution.
  • At value  equal to 7 the solution is said to be neutral.

pOH=-\log[OH^-]

pOH=-\log[5.5\times 10^{-5} M]=4.259

pH +pOH = 14

pH = 14-pOH

pH=14 - 4.259 = 9.741

The pH of the solution is defined as negative logarithm of hydronium ions of in an aqueous solution.

  • Higher the value of pH more will be the basic solution.
  • Lower the value of pH more will be the acidic solution.
  • At value equal to 7 the solution is said to be neutral.

pH=-\log[H_3O^+]

9.741=-\log[H_3O^+]

[H_3O^+]=1.8\times 10^{-10} M

The solution is basic as pH of the solution is 9.741.

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1 year ago
Why do electrons flow through a wire?
I am Lyosha [343]

Answer:

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Explanation:

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3 years ago
Which best describes the result of tropical continental climate in the summer A.hot and sunny B.cool and cloudy
marysya [2.9K]
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6 0
3 years ago
A sample of ammonia ^NH3h gas is completely decomposed to nitrogen and hydrogen gases over heated iron wool. If the total pressu
icang [17]

Answer : The partial pressure of N_2 and H_2 is, 216.5 mmHg and 649.5 mmHg

Explanation :

According to the Dalton's Law, the partial pressure exerted by component 'i' in a gas mixture is equal to the product of the mole fraction of the component and the total pressure.

Formula used :

p_i=X_i\times p_T

X_i=\frac{n_i}{n_T}

So,

p_i=\frac{n_i}{n_T}\times p_T

where,

p_i = partial pressure of gas

X_i = mole fraction of gas

p_T = total pressure of gas

n_i = moles of gas

n_T = total moles of gas

The balanced decomposition of ammonia reaction will be:

2NH_3\rightarrow N_2+3H_2

Now we have to determine the partial pressure of N_2 and H_2

p_{N_2}=\frac{n_{N_2}}{n_T}\times p_T

Given:

n_{N_2}=1\\\\n_{H_2}=3\\\\n_{T}=4\\\\p_T=866mmHg

p_{N_2}=\frac{1}{4}\times (866mmHg)=216.5mmHg

and,

p_{H_2}=\frac{n_{H_2}}{n_T}\times p_T

Given:

n_{H_2}=1\\\\n_{H_2}=3\\\\n_{T}=4\\\\p_T=866mmHg

p_{H_2}=\frac{3}{4}\times (866mmHg)=649.5mmHg

Thus, the partial pressure of N_2 and H_2 is, 216.5 mmHg and 649.5 mmHg

5 0
3 years ago
A container holds 15.0 g of phosphorous gas at a pressure of 2.0 atm and a temperature of 20.0 Celsius. What is the density of t
erik [133]
<span>Density is a value for mass, such as kg, divided by a value for volume, such as m3. Density is a physical property of a substance that represents the mass of that substance per unit volume. We calculate as follows:

PV = nRT
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m/V = P(molar mass)/RT
Density = P(molar mass)/RT 
Density = 2.0 ( 30.97 ) / 0.08206 ( 20 + 273.15) = 2.57 g/L <----First option</span>
5 0
3 years ago
Read 2 more answers
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