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3 years ago

¿Qué pasaría si un organismo o animal fuera eliminado de una red alimentaria?

Chemistry

1 answer:

34kurt3 years ago

4 0

Answer: Sí

Explanation: Sí

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Please help- thank you-

Flauer [41]

Dang that’s crazy.. Goodluck ..

4 0

2 years ago

Read 2 more answers

Which amount of a compound dissolved in 100g of water at the stated temperature represents a solution that is saturated

Assoli18 [71]

40 g KNO, at 25°C

Brainlist?

5 0

2 years ago

Three players (A, B and C) shoot three arrows at a target

UkoKoshka [18]

Answer:

Player B

Explanation:

I just did it and I got it right :)

6 0

2 years ago

Calculate the pKa of lactic acid (CH3CH(OH)COOH) given the following information. 3.005 grams of potassium lactate are added to

snow_lady [41]

Answer:

$\displaystyle \text{p} K_a \approx 3.856$

Explanation:

Because 3.005 grams of potassium lactate is added to 100. mL of solution, its concentration is:

$\displaystyle \begin{aligned} \left[ \text{KC$_3$H_$_5$O$_3$}\right] & = \frac{3.005\text{ g KC$_3$H_$_5$O$_3$}}{100.\text{ mL}} \cdot \frac{1\text{ mol KC$_3$H_$_5$O$_3$}}{128.17 \text{ g KC$_3$H_$_5$O$_3$}} \cdot \frac{1000\text{ mL}}{1\text{ L}} \\ \\ &= 0.234\text{ M}\end{aligned}$

By solubility rules, potassium is completely soluble, so the compound will dissociate completely into potassium and lactate ions. Therefore, [KC₃H₅O₃] = [C₃H₅O₃⁺]. Note that lactate is the conjugate base of lactic acid.

Recall the Henderson-Hasselbalch equation:

$\displaystyle \begin{aligned}\text{pH} = \text{p}K_a + \log \frac{\left[\text{Base}\right]}{\left[\text{Acid}\right]} \end{aligned}$

[Base] = 0.234 M and [Acid] = 0.500 M. We are given that the resulting pH is 3.526. Substitute and solve for pKₐ:

$\displaystyle \begin{aligned} (3.526) & = \text{p}K_a + \log \frac{(0.234)}{(0.500)} \\ \\ 3.526 & = \text{p}K_a + (-0.330) \\ \\ \text{p}K_a & = 3.856\end{aligned}$

In conclusion, the pKₐ value of lactic acid is about 3.856.

5 0

1 year ago

A chemist prepares a solution by dissolving 0.3 mole of CaCl2 in enough water to make 1000 mL of solution. What is the molar con

Rasek [7]

$CaCl_{2}$ dissolves in water to give $Ca^{2+}$ and $Cl^{-}$ ions according to the following reaction:

$CaCl_{2}$ --------> $Ca^{2+}$ + 2 $Cl^{-}$

So, according to the above reaction, 1 mole of $CaCl_{2}$ produce 2 moles of $Cl^{-}$ ion,

So, 0.3 mole will give = 0.3 x 2 = 0.6 moles of $Cl^{-}$ ion

So, Molar concentration = $\frac{0.6moles}{1L} = 0.6$

Note: 1L = 1000mL

7 0

2 years ago