3 years ago

Which of the following is true regarding the law of conservation of mass?

Chemistry

1 answer:

nexus9112 [7]3 years ago

8 0

A is correct................

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Suppose you put a whole antacid tablet in one glass of water and a crushed antacid tablet in another glass containing the same a

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The crushed tablets would stop bubbling/fuzzing first because it has a smaller surface area which means that it would dissolve before the uncrushed tablets which has a larger surface area.

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OS-182 has a half-life of 3.6 days. If a sample started at 175 grams, how much would be led after 18 days?

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Calculate the value of AE for a system that loses 50 J of heat and has 150 J of work Performed on it by the surroundings.

gavmur [86]

Answer:

100 j

Explanation:

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What is the formula for hydrogen-hydrogen?

kupik [55]

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Calculate the pH for the following weak acid. A solution of HCOOH has 0.12M HCOOH at equilibrium. The Ka for HCOOH is 1.8×10−4.

Shtirlitz [24]

Answer:

the pH of HCOOH solution is 2.33

Explanation:

The ionization equation for the given acid is written as:

$HCOOH\leftrightarrow H^++HCOO^-$

Let's say the initial concentration of the acid is c and the change in concentration x.

Then, equilibrium concentration of acid = (c-x)

and the equilibrium concentration for each of the product would be x

Equilibrium expression for the above equation would be:

$\Ka= \frac{[H^+][HCOO^-]}{[HCOOH]}$

$1.8*10^-^4=\frac{x^2}{c-x}$

From given info, equilibrium concentration of the acid is 0.12

So, (c-x) = 0.12

hence,

$1.8*10^-^4=\frac{x^2}{0.12}$

Let's solve this for x. Multiply both sides by 0.12

$2.16*10^-^5=x^2$

taking square root to both sides:

$x=0.00465$

Now, we have got the concentration of $[H^+] .$

$[H^+] = 0.00465 M$

We know that, $pH=-log[H^+]$

pH = -log(0.00465)

pH = 2.33

Hence, the pH of HCOOH solution is 2.33.

7 0

3 years ago

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