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Alborosie
3 years ago
15

Help! I will mark you the brainest !! ☺️☺️

Mathematics
1 answer:
Marizza181 [45]3 years ago
3 0

Answer:

Part 1)  0.675\%

Part 2) 475\%

Part 3) 8\%

Part 4) \frac{67}{20}

Part 5) 2.65

Step-by-step explanation:

Part 1) Write as a percent 0.00675

we know that

To write a number as a percent, multiply the number by 100

so

0.00675*100=0.675\%

Part 2) Write as a percent 4 3/4

Convert mixed number to an improper fraction

4\frac{3}{4}=\frac{4*4+3}{4}=\frac{19}{4}

we know that

To write a fraction as a percent, multiply the fraction by 100

\frac{19}{4}*100=19*25=475\%

Part 3) Write as a percent 2/25

we know that

To write a fraction as a percent, multiply the fraction by 100

\frac{2}{25}*100=2*4=8\%

Part 4) write as a fraction 335%

we know that

335\%=\frac{335}{100}

Simplify

Divide by 5 both numerator and denominator

\frac{335}{100}=\frac{67}{20}

Part 5) Write as a decimal 265%

we know that

265\%=\frac{265}{100}=2.65

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Answer:

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4 0
3 years ago
Butyric acid ( c3h7cooh) is a weak acid . what is the ph of a 0.0250 m solution of this acid. ka = 1.5 x 10-5 (2 decimal places)
Wewaii [24]

The pH of the weak acid is 3.21

Butyric acid is known as a weak acid, we need the concentration of [H+] formula of weak acid which is given by this equation :

[H^{+}]=\sqrt{Ka . Ma}

where [H+] is the concentration of ion H+, Ka is the weak acid ionization constant, and Ma is the acid concentration.

Since we know the concentration of H+, the pH can be calculated by using

pH = -log[H+]

From question above, we know that :

Ma = 0.0250M

Ka = 1.5 x 10¯⁵

By using the equation, we can determine the concentration of [H+]

[H+] = √(Ka . Ma)

[H+] = √(1.5 x 10¯⁵ . 0.0250)

[H+] = 6.12 x 10¯⁴ M

Substituting the value of [H+] to get the pH

pH = -log[H+]

pH = -log(6.12 x 10¯⁴)

pH = 3.21

Hence, the pH of the weak acid c3h7cooh is 3.21

Find more on pH at: brainly.com/question/14466719

#SPJ4

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1 year ago
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Step-by-step explanation:

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