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aksik [14]
1 year ago
14

How many grams of solute would you use to prepare the following solutions?241.0 mL of 1.11 M NaOHExpress your answer with the ap

propriate units.
Chemistry
1 answer:
Ludmilka [50]1 year ago
8 0
<h2>Answer:</h2>

10.7 grams

<h2>Explanations:</h2>

The formula for calculating the molarity of a solution is given as:

\begin{gathered} molarity=\frac{moles}{volume} \\ moles=molarity\times volume \end{gathered}

Given the following parameters

molarity of NaOH = 1.11M

volume of solution = 241.0mL = 0.241L

Find the moles of NaOH

\begin{gathered} moles\text{ of Na}OH=\frac{1.11mol}{L}\times0.241L \\ moles\text{ of Na}OH=0.2675moles \end{gathered}

Determine the mass of solute (NaOH)

\begin{gathered} Mass\text{ of NaOH}=mole\times molar\text{ mass} \\ Mass\text{ of NaOH}=0.2675\times40 \\ Mass\text{ of NaOH}=10.7grams \end{gathered}

Hence the grams of solute that would be used to prepare the solution is 10.7grams

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When the amount of gas in a container is increased, the volume increases. Lussac's law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.

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I have a 4 amino acid peptide of unknown sequence with a curious titration profile around pH = 6. If Iknow that the peptide N-te
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c. Histidine

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A sample of N2 gas in a flask is heated from 27 Celcius to 150 Celcius. If the original gas is @ pressure of 1520 torr, what is
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Answer:

\large \boxed{\text{B.) 2.8 atm}}

Explanation:

The volume and amount are constant, so we can use Gay-Lussac’s Law:

At constant volume, the pressure exerted by a gas is directly proportional to its temperature.

\dfrac{p_{1}}{T_{1}} = \dfrac{p_{2}}{T_{2}}

Data:

p₁ = 1520 Torr; T₁ =   27 °C

p₂ = ?;               T₂ = 150 °C

Calculations:

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T₁ = (  27 + 273.15) K = 300.15 K

T₂ = (150 + 273.15) K = 423.15 K

(b) Calculate the new pressure

\begin{array}{rcl}\dfrac{1520}{300.15} & = & \dfrac{p_{2}}{423.15}\\\\5.064 & = & \dfrac{p_{2}}{423.15}\\\\5.064\times423.15&=&p_{2}\\p_{2} & = & \text{2143 Torr}\end{array}\\

(c) Convert the pressure to atmospheres

p = \text{2143 Torr} \times \dfrac{\text{1 atm}}{\text{760 Torr}} = \textbf{2.8 atm}\\\\\text{The new pressure reading will be $\large \boxed{\textbf{2.8 atm}}$}

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A teacher makes the following statement.
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Read 2 more answers
A rectangular block has the following dimensions: 3.21 dm, 5.83 cm, and 1.84 in. The block has a mass of 1.94 kg. What is the de
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The density of the rectangular block in g/mL is 7.0.

<u>Given the following data:</u>

  • Mass of block = 22.8 gra1.94 kg
  • Length of block = 3.21 cm
  • Width of block = 5.83 cm
  • Height of block = 1.84 in.

To find the density of the block in g/mL:

First of all, we would determine the volume of the rectangular block by using the following formula:

Volume = length × width × height

<u>Conversion:</u>

1 in = 2.54 cm​

5.83 in = X cm

Cross-multiplying, we have:

X = 2.54(5.83)\\\\X = 14.81 \; cm

Volume = 3.21 × 5.83 × 14.81

Volume = 277.16 cubic centimeters.

<u>Note</u>: Milliliter (mL) is the same as cubic centimeters.

1000 grams = 1 kg

Y grams = 1.94 kg

Cross-multiplying, we have:

Y = 1940 grams

Now, we can find the density:

Density = \frac{Mass}{Volume}\\\\Density = \frac{1940}{277.16}

<em>Density </em><em>= 7</em><em>.0 g/mL</em>

Therefore, the density of the rectangular block in g/mL is 7.0.

Read more: brainly.com/question/18320053

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