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2 years ago

6

You are on a field trip to a nearby lake for biology class and want to perform a quick analysis of the water’s approximate pH le

vel. Which pH measurement system would you use and why?

2 answers:

sp2606 [1]2 years ago

7 0

Sample Response: Using pH paper would be best for doing a quick measurement in the field. It does not need to be calibrated and the papers provide an instant estimate. Answer on Ed

umka21 [38]2 years ago

4 0

The easiest way to approximate ph level is the ph paper because there are no exprimentation required and it is very handy. so it is the best way to approximate the ph level of a lake, especially when you are outdoors, and it is just an initial reading of the ph. so ph paper will do.

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How many moles of NH3 from when 32.4 L of H2 gas completely reacts at STP according to the following reaction? Remember 1 mol of

Travka [436]

N_2 (g) + 3H_2 (g) rightarrow 2NH_3 (g) volume of H_2 = 32.44 At STP 1 mole of H_2 = 22.4L ? mole of H_2 = 32.4L therefore moles of H_2

8 0

2 years ago

Calculate the mass of 25,000 molecules of nitrogen gas. (1 mole = 6.02 x 1023 molecules)

Ainat [17]

Hey there!

Molar mass N2 = 28.01 g/mol

Therefore:

28.01 g N2 -------------- 6.02*10²² molecules N2

( mass N2 ?? ) ----------- 25,000 molecules N2

mass N2 = ( 25,000 * 28.01 ) / ( 6.02*10²³ )

mass N2 = 700250 / 6.02*10²³

mass N2 = 1.163*10⁻¹⁸ g

Hope that helps!

7 0

2 years ago

Read 2 more answers

Consider the structure of the amino acid alanine. indicate the hybridization about each interior atom.

OLEGan [10]

The structure of Alanine is shown below,
Except the carbon atom of carbonyl group which is Sp² Hybridized, all remaining atoms are Sp³ Hybridized. The hybridization of each element is depicted in a box below,

5 0

2 years ago

Read 2 more answers

What would be the composition and ph of an ideal buffer prepared from lactic acid (ch3chohco2h), where the hydrogen atom highlig

Mashutka [201]

Answer:

$P_H =2.86$

$c=1.4\times 10^{-4}$

Explanation:

first write the equilibrium equaion ,

$C_3H_6O_3$ ⇄ $C_3H_5O_3^{-} +H^{+}$

assuming degree of dissociation $\alpha$ =1/10;

and initial concentraion of $C_3H_6O_3$ =c;

At equlibrium ;

concentration of $C_3H_6O_3 = c-c\alpha$

$[C_3H_5O_3^{-} ]= c\alpha$

$[H^{+}] = c\alpha$

$K_a = \frac{c\alpha \times c\alpha}{c-c\alpha}$

$\alpha$ is very small so $1-\alpha$ can be neglected

and equation is;

$K_a = {c\alpha \times \alpha}$

$[H^{+}] = c\alpha$ = $\frac{K_a}{\alpha}$

$P_H =- log[H^{+} ]$

$P_H =-logK_a + log\alpha$

$K_a =1.38\times10^{-4}$

$\alpha = \frac{1}{10}$

$P_H= 3.86-1$

$P_H =2.86$

composiion ;

$c=\frac{1}{\alpha} \times [H^{+}]$

$[H^{+}] =antilog(-P_H)$

$[H^{+} ] =0.0014$

$c=0.0014\times \frac{1}{10}$

$c=1.4\times 10^{-4}$

6 0

2 years ago

Why the gross reading is needed when doing the titration?

aleksklad [387]

Answer:

The answer is below

Explanation:

Because various factors can affect the actual value of the titration outcome. Some of these factors can range from errors from a researcher also known as human error, misreading the quantities, researcher's perception of the color, or wrong procedure in carrying out the experimentation.

Hence, in order to avoid such error, a researcher needs to be thorough during the process of experimentation, and using gross reading can help to avoid these errors when the titre value is eventually determined.

7 0

2 years ago