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skelet666 [1.2K]
1 year ago
8

PLEASE HURYYYYY!

Chemistry
1 answer:
Ainat [17]1 year ago
6 0

The variables and constants will be:

1. Dependent variable: Plant growth expressed as height

2. A different temperature-an independent variable

3. Constant variables: the quantity and quality of water, sunlight, and soil.

<h3>What would your constants be, as well as your variables?</h3>

The independent, dependent, and constant variables are the three categories of variables that must be present in a scientific experiment.

1. Independent variable: A variable that can be altered or changed manually or on its own. The examined variable is directly influenced by the variable. The varying temperature that is given to the plants in the particular situation is the independent variable.

2. Dependent variable- The growth of the plant, which is assessed in terms of height, is the variable that is being researched in the experiment and directly influenced by the independent variable.

3. Constant variable – The variable that is maintained constant during the experiment and does not change, such as the quantity of water used, the amount of sunlight received, or the kind of soil.

To know more about constant variable visit: brainly.com/question/20693695

#SPJ4

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What is the pH when 10.0 mL of 0.20 M potassium hydroxide is added to 30.0 mL of 0.10 M cinnamic acid, HC9H7O2 (Ka = 3.6 × 10–5)
astra-53 [7]

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Solution:- As is clear from the given Ka value, Cinnamic acid is a weak acid. let's calculate the moles of acid and KOH added to it from their given molarities and mL.

For KOH,  10.0mL(\frac{1L}{1000mL})(\frac{0.20mol}{1L})

= 0.002 mol

For Cinnamic acid,  30.0mL(\frac{1L}{1000mL})(\frac{0.10mol}{1L})

= 0.003 mol

Acid and base react as:

HC_9H_7O_2(aq)+KOH(aq)\rightleftharpoons KC_9H_7O_2(aq)+H_2O(l)

The reaction takes place in 1:1 mol ratio. Since the moles of acid are in excess, the acid is still remaining when all the kOH is used.

0.002 moles of KOH react with 0.002 moles of Cinnamic acid to form 0.002 moles of potassium cinnamate. Excess moles of Cinnamic acid = 0.003 - 0.002 = 0.001

As the solution have weak acid and it's salt(or we could say conjugate base), it is a buffer solution and the pH of the buffer solution could easily be calculated using Handerson equation:

pH=pKa+log(\frac{base}{acid})

pKa could be caluted from given Ka value using the formula:

pKa = - log Ka

pKa=-log3.6*10^-^5

pKa = 4.44

let's plug in the values in Handerson equation and calculate the pH:

pH=4.44+log(\frac{0.002}{0.001})

pH = 4.44+0.30

pH = 4.74

So, the first choice is correct, pH is 4.74.

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3 years ago
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