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4 years ago

I'm not sure which category this is. But please help me on this!!

Chemistry

1 answer:

MrRissso [65]4 years ago

8 0

Answer:

Tom

Explanation:

Simply because we see Claudia used a shortcut. Tom uses more physical force than Claudia, since Claudia only had to push the boxes into there required shelves.

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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.

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3 years ago

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Below the ecosystem is soil, granted, and bedrock. however for the ocean ecosystem has sand below it.

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Elena-2011 [213]

Answer:

both iodine

Explanation:

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4 years ago

Which subshell is represented by the lanthanides family

balu736 [363]

Subshell f is represneted

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3 years ago

A 3.0 L solution contains 73.5 g of H2SO4. Calculate the molar concentration of the solution.

kozerog [31]

$C_{m}=\frac{m}{MV}=\frac{73,5g}{98\frac{g}{mol}*3L}=0,25M\\\\
C_{1}V_{1}=C_{2}V_{2}\\\\
0,25M*3L=0,18M*V_{2}\\\\
V_{2}=\frac{0,25M*3L}{0,18M}\approx 4,17L\\\\
4,17L-3L=1,17L$

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4 years ago