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guajiro [1.7K]
3 years ago
12

Why do scientists consider any hypothesis valuable?

Chemistry
1 answer:
Serjik [45]3 years ago
3 0

Answer:

I hope this answer is correct

Explanation:

A hypothesis requires no further investigation if it is proved by the experiment.

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Determine the [OH-], pH, and pOH of a solution with a [H+] of 0.090 M at 25 °C. [OH-] = pH = pOH = 0 POH =
ValentinkaMS [17]

Answer : The concentration of OH^- ion, pH and pOH of solution is, 1.12\times 10^{-13}M, 1.05 and 12.95 respectively.

Explanation : Given,

Concentration of H^+ ion = 0.090 M

pH : It is defined as the negative logarithm of hydrogen ion or hydronium ion concentration.

The expression used for pH is:

pH=-\log [H^+]

First we have to calculate the pH.

pH=-\log [H^+]

pH=-\log (0.090)

pH=1.05

The pH of the solution is, 1.05

Now we have to calculate the pOH.

pH+pOH=14\\\\pOH=14-pH\\\\pOH=14-1.05=12.95

The pOH of the solution is, 12.95

Now we have to calculate the OH^- concentration.

pOH=-\log [OH^-]

12.95=-\log [OH^-]

[OH^-]=1.12\times 10^{-13}M

The OH^- concentration is, 1.12\times 10^{-13}M

5 0
2 years ago
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How is a rainbow made
MaRussiya [10]
You could look that up-
5 0
2 years ago
Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.45 M of reagent
sladkih [1.3K]

Answer:

\large\boxed{\large\boxed{0.0014M/s}}

Explanation:

From the table, first find the order of reaction, then find the rate constant, write the rate equation, and, finally, subsititue the data for the reaction that starts with 0.45M of reagent A and 0.90 M of reagents B and C.

<u>1. Table</u>

Trial  [A] (M)    [B] (M)   [C] (M)    Initial rate (M/s)

 1        0.20      0.20       0.20         6.0×10⁻⁵

2        0.20      0.20       0.60         1.8×10⁻⁴

3        0.40      0.20        0.20        2.4×10⁻⁴

4        0.40      0.40        0.20        2.4×10⁻⁴

<u>2. Orders</u>

a) From trials 3 and 4 you learn that the initial concentration of B does not change the change teh rate of the reaction. Hence the order with respect to [B] is 0.

b) From trials 1 and 2 you learn that when the concentration of C is tripled the rate of reaction is also tripled:

  • 0.60 / 0.2 = 3, and
  • 1.8×10⁻⁴ / 6.0×10⁻⁵ = 3

Hence, the order with respect to C is 1.

c) From trials 1 and 3 you get:

  • 0.40/0.2 = 2
  • 2.4×10⁻⁴ /  6.0×10⁻⁵ = 4

Which means that when the concentration of A is doubled, the rate of the reaction is quadruplicated. Hence, the order of the reaction with respect to A is 2.

<u>3. Rate equation</u>

Ther orders are:

              a=2\\\\b=0\\\\c=1

Hence the rate is:

            rate=k[A]^a{B}^b[C]^c\\ \\ rate=k[A]^2[B]^0[C]^1=k[A]^2C

<u>4. Rate constant, k</u>

<u />

You can use any trial to find the value of the constant, k

Using trial 1:

            6.0\times 10^{-5}M/s=k(0.20M)^2(0.20M)\\ \\ k=\frac{6.0\times 10^{-5}M/s}{(0.20M)^2(0.20M)}=0.0075M^{-2}s^{-1}

<u>5. Rate law:</u>

       rate=k[A]^2C=0.0075[A]^2[C]

<u>6. Substitute</u>

Subsititue the data for the reaction that starts with 0.45M of reagent A and 0.90 M of reagents B and C.

        rate=0.0075M^{-2}s^{-1}[A]^2[C]=0.0075M^{-2}s^{-1}[0.45M]^2[0.9M]

        r=0.00136688M/s\approx 0.0014M/s

7 0
3 years ago
You cannot round a number if it has a decimal point true or false
Katyanochek1 [597]
The answer is false. u can still round if # is a decimal
5 0
3 years ago
Aqueous humor forms during capillary filtration in the __________?
Karolina [17]

Answer:

Ciliary body.

Explanation:

Ciliary body: It is the known for the part of the eye that includes the ciliary muscle, which helps in the control the ciliary epithelium and lens shape, which are helping in the production of aqueous humor.

Through active secretion mechanism helping in to produce eighty percent of aqueous humor, and through the plasma ultra-filtration mechanism twenty percent of aqueous humor is produced.

Ciliary body is the part of the layer which helps to deliver the nutrients, and oxygen to the eye tissues, and this layer is known as uvea.

7 0
3 years ago
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