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3 years ago

The forces exerted on an object are shown.

Chemistry

2 answers:

marusya05 [52]3 years ago

7 0

Answer:

The object moves up.

Explanation:

I think that's the answer because since F was up that would cause 5 N . To go up.

Tell me if I'm wrong, plz :D

Juliette [100K]3 years ago

4 0

Answer:

The object moves up

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The density of mercury is 13.5 g/ml and the density of water is 1.00 g/ml. if a mercury barometer reads 709 mmhg, what is the ba

lesya [120]

Go to the chem text book

3 0

3 years ago

What is the solution to the problem expressed to the correct number of significant figures? 2.13 + 1 = ?

Paha777 [63]

So,

With addition, we the last digit we keep will be the one which is known for both individual values.

We know 2.13 to the hundredths, but we only know 1 to the ones. Therefore, we will round off in the ones place.

2.13 + 1 = 3.13 (unrounded)

= 3 (rounded)

Hope this helps!

7 0

3 years ago

What is the pH of a 3.5 x 10-^6 M solution of HCl?

Svetach [21]

Answer:

5.46

Explanation:

From the question,

pH this can be defined as the acidity or alkalinity of a solution.

The expression for pH is given as

pH = -log(H⁺)...................... Equation 1

Where H⁺ = Hydrogen ion of HCL

Given: H⁺ = 3.5×10⁻⁶ M

Substitite this value into equation 1

pH = -log(3.5×10⁻⁶)

pH = 5.46

Hence the pH of HCl is 5.46

8 0

3 years ago

On the basis of molecular structure and bond polarity, which of the following compounds is most likely to have the greatest solu

Drupady [299]

Answer:

$\boxed{\text{c) NH$_{3}$; hydrogen bonding}}$

Explanation:

For each of these molecules, you must determine their VSEPR structure and then identify the strongest intermolecular forces.

Remember that water is a highly polar molecule.

a) CH₄

Electron geometry: tetrahedral

Molecular geometry: tetrahedral

Bond polarity: C-H bond nonpolar

Molecular polarity: nonpolar

Strongest IMF: London dispersion forces

Solubility in water: low

A nonpolar molecule is insoluble in a polar solvent.

b) CCl₄

Electron geometry: tetrahedral

Molecular geometry: tetrahedral

Bond polarity: C-Cl bond nonpolar

Molecular polarity: nonpolar (symmetrical molecule. All bond dipoles cancel)

Strongest IMF: London dispersion forces

Solubility in water: low

A nonpolar molecule is insoluble in a polar solvent.

d) PH₃

Electron geometry: tetrahedral

Molecular geometry: trigonal pyramidal

Bond polarity: P-H bonds are polar

Molecular polarity: polar (all P-H bond dipoles point towards P)

Strongest IMF: dipole-dipole

Solubility in water: soluble

A polar molecule is soluble in a polar solvent.

c) NH₃

Electron geometry: tetrahedral

Molecular geometry: trigonal pyramidal

Bond polarity: N-H bonds are highly polar

Molecular polarity: highly polar (all N-H bond dipoles point towards N)

Strongest IMF: hydrogen bonding

Solubility in water: highly soluble

NH₃ is so polar that it can form hydrogen bonds with water.

$\boxed{\textbf{The compound with the greatest solubility in water is NH$_{3}$}}$

8 0

3 years ago

A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that fo

amid [387]

Explanation:

Ksp of NiCO3 = 1.4 x 10^-7

Ksp of CuCO3 = 2.5 x 10^-10

Ionic equations:

NiCO3 --> Ni2+ + CO3^2-

CuCO3 --> Cu2+ + CO3^2-

[Cu2+][CO3^2-]/[Ni2+][CO3^2-]

= (2.5* 10^-10)/(1.4* 10^-7)

= 0.00179.

[Cu2+]/[Ni2+]

= 0.00179

= 0.00179*[Ni2+]

If all of Cu2+ is precipitated before Na2CO3 is added.

= 0.00179 * (0.25)

The amount of Cu2+ not precipitated = 0.000448 M

The percent of Cu2+ precipitated before the NiCO3 precipitates = concentration of Cu2+ unprecipitated/initial concentration of Cu2+ * 100

= 0.000448/0.25 * 100

= 0.18%

Therefore, percentage precipitated = 100 - 0.18

= 99.8%

The two metal ions can be separated by slowly adding Na2CO3. Thus that is the unpptd Cu2+.

8 0

3 years ago