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2 years ago

14

If the H+ ion concentrati on in an aqueous solution is 0.0010 M, why is it not possible for the OH− ion concentration to be 1.0

× 10−10M?

1 answer:

spayn [35]2 years ago

6 0

Answer:

im not sure sry

Explanation:

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Explain how an equation can be balanced even if the number of reactant particles differs from the number of product particles

swat32

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Add coefficients in front of the products and/or reactants to get the same amount of particles on both side</span>

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3 years ago

An isotope of cesium (cesium-137) has a half-life of 30 years. If 1.0 g of cesium-137 disintegrates over a period of 90 years, h

Anestetic [448]

Answer:

3 half-lives 7. An isotope of Cesium (Cesium-137) has a half life of 30 years. If 1.0 mg of cesium-137 disintegrates over a period of 90 years, how many mg of cesium-137 would remain? of sodium-25 is 60 seconds? : 3 minutes t=601 = 3 half-lives 5.0mg ~ 2.5 mg + 1.25mg →) 625 mg.

Explanation:

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3 years ago

Why is accidental overlap of signals much more common in H-1 NMR than in C-13 NMR?

alexdok [17]

Answer:

See explanation

Explanation:

Accidental overlap of signals are common in H-1 NMR than in C-13 NMR for the following reasons;

1) 13C has a very low natural abundance compared to H-1

2) 13C nucleus is s many times lesser in NMR sensitivity than H-1 nucleus.

3) As a result of its low abundance, 13C-13C coupling is not common.

4) Longer relaxation times do not give room for integrations.

5) Peaks in 13C spectra mainly consists of single lines.

As a result of all these, 13C-NMR spectra take longer to acquire than H-NMR. Hence, accidental overlap of signals is much more common in H-1 NMR than in C-13 NMR.

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3 years ago

What is the pressure, in mmhg, of a 4.00 g sample of o2 gas, which has a temperature of 30.0 °c, and a volume of 3000 ml?

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Answer:- Pressure of the gas is 790.4 mmHg.

Solution:- Mass of the gas oxygen gas is 4.00 g, temperature is 30.0 degree C and volume is 3000 mL and it asks to calculate the pressure of the gas.

It is based on ideal gas law equation, PV = nRT

Where, P is pressure, V is volume, n is number of moles, R is the universal gas constant and T is temperature.

Let's convert the mass to moles on dividing the grams by molar mass. Molar mass of oxygen is 32 gram per mol.

n = $4.00g(\frac{1mol}{32g})$

n = 0.125 moles

Convert degree C to kelvin, for this we add 273.

T = 30.0 + 273 = 303 K

Convert mL to L. For this we divide the given volume by 1000.

V = $3000mL(\frac{1L}{1000mL})$

V = 3 L

Value of R is 0.0821 atm.L per mol per K.

The equation is rearranged for the pressure as:

$P=\frac{nRT}{V}$

Let's plug in the values in the equation to calculate the pressure, P.

$P=\frac{0.125*0.0821*303}{3}$

P = 1.04 atm

They want answer in mmHg, so let's convert the pressure unit from atm to mmHg.

1 atm = 760 mmHg

so, $1.04atm(\frac{760mmHg}{1atm})$

= 790.4 mmHg

So, the pressure of the gas is 790.4 mmHg.

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3 years ago

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Carbohydrates should be your answer.

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3 years ago