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2 years ago

Lab report on flock flock y flock z insects and fruits

Chemistry

1 answer:

n200080 [17]2 years ago

7 0

Answer:

In this lab, you will learn the anatomy of an insect, how to identify an insect to order, how to collect and curate insects,

Explanation:

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Tomato juice has a pH of 4.20. Calculate the [H3O+] and [OH–] in tomato juice.

Free_Kalibri [48]

[H3O+] = 10^(-pH) = 10^(-4.20) = 6.3 x 10^-5 M

pOH = 14 - pH = 14 - 4.20 = 9.80

[OH-] = 10^(-pOH) = 10^(-9.80) = 1.6 x 10^-10 M

8 0

3 years ago

How many liters of a 0.30M solution are needed to give 2.7 moles of solute? Your answer:

OverLord2011 [107]

You HAVE TO know that molarity (M) tells you the number of moles of a solute per Liters of solution.
M=mol/L
0.3M = 2.7 mol/ Volume
Volume = 2.7 mol/3.0 L
Volume = 0.9 L

8 0

4 years ago

Read 2 more answers

Why are some metals reactive than others?

Naddik [55]

some elements have their outer electrons more tightly bound than others. Those who have less tightly bound electrons are more reactive. After this it gets more complex in explaining why they are bound with different strengths.

7 0

3 years ago

Read 2 more answers

In a 1.0× 10–6 M solution of Ba(OH)2(aq) at 25 °C, identify the relative molar amounts of these species.

Marysya12 [62]

Thank you for posting your question here. Below is the solution:

HNO3 --> H+ + NO3-
HNO3 = strong acid so 100% dissociation 
** one doesn't need to find the molarity of water since it is the solvent 

0M HNO3 
1x10^-6M H3O+ 
1x10^-6M NO3- 
1x10^-8M OH-.....the Kw = 1x10^-14 = [H+][OH-] 
you have 1x10^-6M H+ so, 1x10^-14 / 1x10^-6 = 1x10^-8M OH- 

1x10^-6 Ba(OH)2 = strong base, 100% dissociation 
1x10^-6M Ba2+ 
2x10^-6M OH- since there are 2 OH- / 1 Ba2+ 
0M Ba(OH)2 
5x10^-9M H3O+

4 0

4 years ago

What volume (in liters) of a solution contains 0.14 mol of KCl?

oksano4ka [1.4K]

Answer:

$\boxed {\boxed {\sf 0.078 \ L }}$

Explanation:

We are asked to find the volume of a solution given the moles of solute and molarity.

Molarity is a measure of concentration in moles per liter. It is calculated using the following formula:

$molarity= \frac{moles \ of \ solute}{liters \ of \ solution}$

We know there are 0.14 moles of potassium chloride (KCl), which is the solute. The molarity of the solution is 1.8 molar or 1.8 moles of potassium chloride per liter.

moles of solute = 0.14 mol KCl
molarity= 1.8 mol KCl/ L
liters of solution=x

Substitute these values/variables into the formula.

$1.8 \ mol \ KCl/ L = \frac { 0.14 \ mol \ KCl}{x}$

We are solving for x, so we must isolate the variable. First, cross multiply. Multiply the first numerator and second denominator, then the first denominator and second numerator.

$\frac {1.8 \ mol \ KCl/L}{1} = \frac{0.14 \ mol \ KCl}{x}$

$1.8 \ mol \ KCl/ L *x = 1*0.14 \ mol \ KCl$

$1.8 \ mol \ KCl/ L *x = 0.14 \ mol \ KCl$

Now x is being multiplied by 1.8 moles of potassium chloride per liter. The inverse operation of multiplication is division, so we divide both sides by 1.8 mol KCl/L.

$\frac {1.8 \ mol \ KCl/ L *x}{1.8 \ mol \ KCl/L} = \frac{0.14 \ mol \ KCl}{1.8 \ mol \ KCl/L}$

$x= \frac{0.14 \ mol \ KCl}{1.8 \ mol \ KCl/L}$

The units of moles of potassium chloride cancel.

$x= \frac{0.14 }{1.8 L}$

$x=0.07777777778 \ L$

The original measurements of moles and molarity have 2 significant figures, so our answer must have the same. For the number we found, that is the thousandth place. The 7 in the ten-thousandth place tells us to round the 7 up to a 8.

$x \approx 0.078 \ L$

There are approximately 0.078 liters of solution.

5 0

3 years ago