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Fudgin [204]
3 years ago
5

A solution has a concetration of 0.3mol/dm3 of sodium hydroxide .what volume of

Chemistry
1 answer:
HACTEHA [7]3 years ago
7 0

Answer:

Ba(OH)2 + H2SO4 ------> BaSO4 + 2H2O

1) Moles of Ba(OH)2 = moles of H2SO4 = 0.025L x 2)0.02M = 5.0 x 10^-4M

Concn of Ba(OH)2 in g/L = 5.0 x 10^-4M x 171.33g/mol = 0.086g/mol

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Marysya12 [62]
I believe the answer is burning a candle
6 0
3 years ago
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What is the pH of a 0.0042 M hydrochloric acid solution?
babymother [125]

Answer:

E) 2.38

Explanation:

The pH of any solution , helps to determine the acidic strength of the solution ,

i.e. ,

  • Lower the value of pH , higher is its acidic strength

and ,

  • Higher the value of pH , lower is its acidic strength .

pH is given as the negative log of the concentration of H⁺ ions ,

hence ,

pH = - log H⁺

From the question ,

the concentration of the solution is 0.0042 M , and being it a strong acid , dissociates completely to its respective ions ,

Therefore , the concentration of H⁺ = 0.0042 M .

Hence , using the above equation , the value of pH can be calculated as follows -

pH = - log H⁺

pH = - log ( 0.0042 M )

pH =  2.38 .

4 0
3 years ago
Write a chemical equation that shows the release of hydroxide ions as each of these bases dissolves in water.
Zarrin [17]
KOH -------> K+ OH-
Ba(OH)2 ------> Ba+2. 2OH-
5 0
3 years ago
Why can some metals be extracted from compounds by heating with carbon and why can some not
pentagon [3]

Answer:

Some metals can be extracted from compounds by heating with carbon atom because they are less reactive than carbon and some metals cannot be extracted because they are more reactive than carbon atom.

Explanation: If the metal is less reactive than carbon atom so the carbon atoms make bond with oxide or other atom present with metal and the metal is free from that oxide or that element. But if the reactivity of metal is higher than carbon is unable to remove the oxide or element.

8 0
3 years ago
At a certain temperature this reaction follows second-order kinetics with a rate constant of 14.1·M−1s−1 : →2SO3g+2SO2gO2g Suppo
RoseWind [281]

Answer:

[SO_3]=0.25M

Explanation:

Hello there!

In this case, since the integrated rate law for a second-order reaction is:

[SO_3]=\frac{[SO_3]_0}{1+kt[SO_3]_0}

Thus, we plug in the initial concentration, rate constant and elapsed time to obtain:

[SO_3]=\frac{1.44M}{1+14.1M^{-1}s^{-1}*0.240s*1.44M}\\\\

[SO_3]=0.25M

Best regards!

4 0
3 years ago
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