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Oxana [17]
3 years ago
10

Bleaching powder was added to excess concentrated hydrochloric acid state whar was observed​

Chemistry
1 answer:
anyanavicka [17]3 years ago
6 0

Answer:

Gas was evolved

Explanation:

The reaction produces chlorine gas which has a pungent smell and is dangerous in excess

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8 0
3 years ago
In a hospital laboratory, a 10.0 mL sample of gastric juice (predominantly HCl), obtained several hours after a meal, was titrat
LiRa [457]

Answer: 1.14

Explanation:

HCl+NaOH\rightarrow NaCl+H_2O

To calculate the molarity of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is HCl

are the n-factor, molarity and volume of base which is NaOH.

We are given:

n_1=1\\M_1=?\\V_1=10.0mL\\n_2=1\\M_2=0.1M\\V_2=7.2mL

Putting values in above equation, we get:

1\times M_1\times 10.0=1\times 0.1\times 7.2\\\\M_1=0.072M

To calculate pH of gastric juice:

molarity of H^+ = 0.072

pH=-log[H^+]

pH=-log(0.072)=1.14

Thus the pH of the gastric juice is 1.14

3 0
3 years ago
A 2.2 M solution is made by with 0.45 moles of a solute. What is the final volume of this solution?
Savatey [412]

Answer: The final volume of this solution is 0.204 L.

Explanation:

Given: Molarity of solution = 2.2 M

Moles of solute = 0.45 mol

Molarity is the number of moles of solute present divided by volume in liters.

Molarity = \frac{no. of moles}{Volume (in L)}

Substitute the values into above formula as follows.

Molarity = \frac{no. of moles}{Volume (in L)}\\2.2 M = \frac{0.45}{Volume}\\Volume = 0.204 L

Thus, we can conclude that the final volume of this solution is 0.204 L.

7 0
3 years ago
Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled.
Shkiper50 [21]

Answer:

  • 0.00358 mol

Explanation:

<u>1) Data:</u>

a) V = 93.90 ml

b) T = 28°C

c) P₁ = 744 mmHg

d) P₂ = 28.25 mmHg

d) n = ?

<u>2) Conversion of units</u>

a) V = 93.90 ml × 1.000 liter / 1,000 ml = 0.09390 liter

b) T = 28°C = 28 + 273.15 K = 301.15 K

c) P₁ = 744 mmHg × 1 atm / 760 mmHg = 0.9789 atm

d) P₂ = 28.5 mmHg × 1 atm / 760 mmHg = 0.0375 atm

<u>3) Chemical principles and formulae</u>

a) The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. Hence, the partical pressure of the hydrogen gas collected is equal to the total pressure less the vapor pressure of water.

b) Ideal gas equation: pV = nRT

<u>4) Solution:</u>

a) Partial pressure of hydrogen gas: 0.9789 atm - 0.0375 atm = 0.9414 atm

b) Moles of hygrogen gas:

pV = nRT ⇒ n = pV / (RT) =

n =  (0.9414 atm × 0.09390 liter) / (0.0821 atm-liter /K-mol × 301.15K) =

n = 0.00358 mol (which is rounded to 3 significant figures) ← answer

7 0
3 years ago
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Does anyone know how to find mass of NaN3?
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The molar mass (atomic weight ) of sodium is 23.0 grams/mole and the molar mass of sodium azide, NaN3 , is the mass of sodium, 23.0 gram/mole added to the molar mass of three atoms of nitrogen (14.0 x 3 = 42 gram/mole) which equals 65.0 grams/mole. The percentage of sodium is 23.0 /65.0 x 100 % = 35 %
4 0
2 years ago
Read 2 more answers
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