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2 years ago

Calculate how many grams of water needed to dissolve 35.00g KNO, at 50.0°C

1 answer:

5 0

Answer:use of significant figures in calculations in Essential Skills 1 () prior to working this example. A Density is mass per unit volume and is usually reported in grams per cubic understand its identity, he found that carbon dioxide dissolved in water to produce compounds were not generally accepted for more than 50 years.

Explanation:

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likoan [24]

Answer:

I think is the last one!!!! punnet square ⬜

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2 years ago

A heated metal object measures 120⁰C. It is dropped into a small bucket filled with water that is 10⁰C. Which of the following i

VARVARA [1.3K]

Answer:

Explanation:

(d the water and metal will adjust to the same temperature between 10 degree c and 120 degree c this temperature will be call equilibrium temperature

7 0

2 years ago

Hello! can a rock transform in to ANY type of rock? and why or why not

Oxana [17]

Answer:

yes it can

Explanation:

because, it depends on where the rock is, for example on a dessert it would Be cracked and things like that if near an eruption it would be the flamey black rock, and so on you get it

3 0

2 years ago

A 275-mL f lask contains pure helium at a pressure of 752 torr. A second f lask with a volume of 475 mL contains pure argon at a

Mashutka [201]

Answer:

The partial pressure of Helium is 275.7 torr

The partial pressure of argon is 457.3 torr

The total pressure is 733 torr

Explanation:

Step 1: Data given

Volume helium flask = 275 mL = 0.275L

Pressure in helium flask = 752 torr

Volume argon flask = 475 mL = 0.475 L

Pressure in argon flask = 722 torr

Step 2: Calculate the total volume of the gas mixture once the stopcock is opened.

Total volume = volume of Helium flask + volume argon flask

Total volume = 275 + 475 = 750 mL = 0.750 L

Step 3: Calculate partial pressure of Helium

pHe *VHe = p'He * Vtotal

⇒ with pHe = the pressure of Helium = 752 torr

⇒ with VHe = the volume in the helium flask = 275 mL

⇒ with p'He = the partial pressure of helium = To be determined

⇒with Vtotal = the total volume = 750 mL

p'He = (pHe*VHe)/Vtotal

p'He = (752*275)/750

p'He = 275.7 torr

Step 4: Calculate partial pressure of Argon

pAr *VAr = p'Ar * Vtotal

⇒ with pAr = the pressure of Argon = 722 torr

⇒ with VAr = the volume in the Argon flask = 475 mL

⇒ with p'Ar = the partial pressure of argon = To be determined

⇒with Vtotal = the total volume = 750 mL

p'Ar = (pAr * VAr)/Vtotal

p'Ar = (722*475)/750

p'Ar = 457.3 torr

Step 5: Calculate the total pressure

Total pressure = partial pressure Helium + partial pressure Argon

Total pressure = 275.7 torr + 457.3 torr = 733 torr

3 0

3 years ago

A buffer can be prepared by mixing two solutions. Determine if each of the following mixtures will result in a buffer solution o

cestrela7 [59]

Answer:

1) A. "Yes, it will result in a buffer solution."

2) A. "Yes, it will result in a buffer solution."

3) A. "No, it will not result in a buffer solution."

4) B. No, it will not result in a buffer solution."

5) B. No, it will not result in a buffer solution.

Explanation:

A buffer system is formed by two components:

A weak acid and its conjugate base.
A weak base and its conjugate acid.

1) Mixing 100.0 mL of 0.1 M HF with 100.0 mL of 0.05 M mol KF. A. "Yes, it will result in a buffer solution."

HF is a weak acid and F⁻ is its conjugate base.

2) Mixing 100.0 mL of 0.1 M NH₃ with 100.0 mL of 0.1 M NH₄Br. A. "Yes, it will result in a buffer solution."

NH₃ is a weak base and NH₄⁺ is its conjugate acid.

3) Mixing 100.0 mL of 0.1 M HCN with 100.0 mL of 0.05 M KOH. A. "No, it will not result in a buffer solution."

It does not have the components of a buffer system.

4) Mixing 100.0 mL of 0.1 M HCl with 100.0 mL of 0.1 M KCl. B. No, it will not result in a buffer solution."

It does not have the components of a buffer system (HCl is a strong acid).

5) Mixing 100.0 mL of 0.1 M HCN with 100.0 mL of 0.1 M KOH. B. No, it will not result in a buffer solution.

It does not have the components of a buffer system.

3 0

3 years ago