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mart [117]
3 years ago
14

0.01 M HCl solution has a pH of 2. Suppose that during the experiment, both the universal pH indicator and the cabbage indicator

turn orange-red for 0.01 M HCl. What can you conclude about the the cabbage indicator key?
Chemistry
4 answers:
evablogger [386]3 years ago
6 0
A) It matches the universal pH indicator and is indicating the proper pH. Yes, this is correct. Have a great day!
NNADVOKAT [17]3 years ago
5 0
It matches the universal pH indicator and is indicating the proper pH
zvonat [6]3 years ago
5 0

Answer:

A ) it matches the universal pH indicator and is indicating the proper pH

Novay_Z [31]3 years ago
4 0
YOU ARE PROBABLY CHEATING RIGHT NOW!!! ... that's cool ig...
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What's an example of using evaporation to separate a mixture in everyday life?
Fed [463]

An example can be perspiration or even rain.

Hope this helps.

8 0
3 years ago
14. All the following are necessary parts of a neutralization reaction except A. an indicator. B. a salt. C. water. D. an acid.
ValentinkaMS [17]

The correct answer is <em>B. a Salt </em><em>because The reaction of an acid and a base is called a neutralization reaction because the properties of both the acid and base are diminished or neutralized when they react. A neutralization reaction is a reaction of an acid with a base in aqueous solution to produce water and a salt, as shown by the following equation:</em>

<em>acid + base → salt + water</em>

<em />

<em>* Hopefully this helps:) Mark me the brainliest:) </em>

<em>∞ 234483279c20∞</em>

6 0
3 years ago
Calculate the percent yield when 500 grams of carbon dioxide react with an excess of water to produce 640 grams of carbonic acid
Elena-2011 [213]

Answer:

Percent yield =  90.5%

Explanation:

Given data:

Mass of carbon dioxide = 500 g

Mass of water = excess

Actual yield of carbonic acid = 640 g

Percent yield = ?

Solution:

Balanced chemical equation:

CO₂ + H₂O  → H₂CO₃

Number of moles of carbon dioxide

Number of moles  = Mass / molar mass

Number of moles = 500 g/ 44 g/mol

Number of moles = 11.4 mol

Now we will compare the moles of H₂CO₃ with CO₂.

                              CO₂          :              H₂CO₃

                                 1             :                  1

                               11.4           :                11.4

Mass of carbonic acid:

Mass = number of moles × molar mass

Mass = 11.4 mol × 62.03 g/mol

Mass = 707.14 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield =  640 g/ 707.14 g × 100

Percent yield =  90.5%

7 0
3 years ago
Help this is due soon!!!
denis23 [38]

Answer:

not 100% sure but I think it's unbalanced chemical

6 0
3 years ago
How many moles are in 300 kilograms of carbon monoxide
QveST [7]

Answer:

Explanation: There are 2 moles of C6H12O6 in 300 g C6H12O6 , rounded to one significant figure.

6 0
2 years ago
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