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3 years ago

An unknown solution has a ph of 8. how would you classify this solution?

1 answer:

6 0

I believe the correct answer from the choices listed above is option C. You would classify this solution as basic since it has the pH of more than 7 which signifies a basic solution. Hope this answers the question. Have a nice day. Feel free to ask more questions.

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All organic compounds have at least ____ carbon and two ____

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All organic compounds have at least 1 carbon and 2 hydrogen atoms.

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2 years ago

What is absolute dating?

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Absolute dating is finding the exact date of an artifact such as a fossil using a technique such as radioactive dating, etc.

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3 years ago

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Imagine if the HCl used in this experiment was prepared at a concentration of 0.150M. Using your calculated volume of HCl neutra

asambeis [7]

Answer:

Molarity = moles / volume

moles of HCl = molarity ×volume

= 0.0150 M × 0.08189L

= 0.0123mol

∴ the amount of CaCO3 neutralized by 0.0123 mole of HCl will be in 1:2 ratio.

moles of CaCO3 = 0.0123 mol of HCl× 1mol CaCO3/ 2mol HCl

= 0 .00614 mol

∴ the tablet has 0.00614 mol of CaCO3.

Explanation:

Step 1:

In the above-experiment problem, HCl acid solution is basically treated with CaCO3 base active in the tablet.

The mass of CaCO3 present in the tablet must be obtained in milligram (mg).

First, write down the balanced reaction between HCl and CaCO3

2Hcl aq + CaC03 s ⇒ CaCl2 aq + H2O l + C02 g

CaCO3 and HCl react in 1:2 ratio of moles respectively.

∴ for each mole of calcium carbonate there would be twice the moles of HCl required for neutralization.

Step 2

the volume is 81.89 mL (i.e 0.08189 L) of 0.150 M HCl neutralizes the whole tablet containing unknown amount of CaCO3.

So, the number of moles of HCl present in the taken volume is calculated

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2 years ago

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If a driver takes 30 min to get to the town market, which is 1.5 km away from his house, what is his average speed?

zvonat [6]

Answer: 0.83 m/s

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1 year ago

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How many grams of AgCl will be produced from 5.00 g of NaCl and 103 g of AgNO3?<br> grams

lapo4ka [179]

Answer:

12.3 g.

Explanation:

Whenever a similar problem is involved, we need to write the chemical reaction representing the net change, as well as due to the fact that we need to know the stoichiometry involved.

Sodium chloride reacts with silver nitrate in a double displacement reaction to produce a cation exchange, that is, we produce silver chloride and sodium nitrate given by the following balanced chemical equation:

$AgNO_3 (aq)+NaCl(aq)\rightarrow AgCl(s)+NaNO_3 (aq)$

According to the balanced chemical equation, the molar stoichiometry of silver nitrate to sodium chloride is 1 : 1.

Let's find moles of each substance to determine the limiting reactant. To do this, divide mass of each component by its molar mass:

$n_{NaCl}=\frac{5.00 g}{58.44 \frac{g}{mol} }= 0.08556 mol\\n_{AgNO_3}=\frac{103 g}{169.87 \frac{g}{mol}}= 0.6063 mol$

Since the stoichiometry of this reaction is 1 : 1, we can compare the moles directly. Notice that the number of moles of NaCl is lower than the number of moles of silver nitrate. This means NaCl is the limiting reactant.

According to the balanced chemical equation, 1 mole of NaCl produces 1 mole of AgCl, so the amount of AgCl would be:

$n_{AgCl}=n_{NaCl}=0.08556 mol$

In order to convert this into mass, let's multiply by the molar mass of AgCl:

$m_{AgCl}=0.08556 mol\cdot143.32 \frac{g}{mol}=12.3 g$

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2 years ago