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2 years ago

1. Which of the following statements describe cations? Select all that apply.

Chemistry

2 answers:

Wittaler [7]2 years ago

5 0

Answer:

<h3>NEGATIVELY CHARGED IONS</h3>

Explanation:

<h2>IHOP NAKATULONG #LIKE AND FOLLOW</h2>

Crazy boy [7]2 years ago

5 0

Hey :)

Cations are positively charged ions and they have lost electrons

Hope this helps!

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Starting with acetylene and bromoethane, show how you would use reagents from the table to synthesize 3-hexanone.

Jobisdone [24]

solution:

A = 192 x (1/2) ^ (15/5) = 192 x (1/2) ^3 = 192 x 1/8 = 24 mg

Starting by hitting acetylene with NaNH2 to deprotonate, this C-- will attack the C connected to the Br Sn2 style to lengthen the chain by two carbons.

Do this same thing again with the other CH of the acetylene and another bromoethaneto get a six carbon chain, namely, 3-hexyne.

Now, reduce the alkyne to an alkene via H2/Pd/C, and that gives 3-hexene.

3 0

3 years ago

A cation with a +4 charge has 26 neutrons and 18 electrons. What is the identity of the element?

Leya [2.2K]

Answer: Titanium has 22 protons

Explanation: If an atoms donates 4 electrons, it forms cation with charge +4. So original atom have 22 electrons and because atom is neutral, it has 22 protons. Number of neutrons does not matter, there are more neutrons than protons in heavier atoms.

3 0

2 years ago

What mass of hbr (in g) would you need to dissolve a 3.4 −g pure iron bar on a padlock?

vivado [14]

Given:

Mass of pure iron (Fe) = 3.4 g

To determine:

Mass of HBr needed to dissolve the above iron

Explanation:

Reaction between HBr and Fe is

Fe + 2HBr → FeBr₂ + H₂

Based on the reaction stoichiometry-

1 mole of Fe reacts with 2 moles of HBr

# moles of Fe = mass of Fe/atomic mass of Fe = 3.4/56 g.mol⁻¹ = 0.0607 moles

Therefore # moles of HBr = 2*0.0607 = 0.1214 moles

Molar mass of HBr = 81 g/mole

Mass of HBr = 0.1214 moles * 81 g/mole = 9.83 g

Ans: Mass of HBR required is 9.83 g

5 0

3 years ago

g If 50.0 mL of a 0.75 M acetic acid solution is titrated with 1.0 M sodium hydroxide, what is the pH after 10.0 mL of NaOH have

V125BC [204]

Answer:

pH = 2.66

Explanation:

Acetic Acid + NaOH → Sodium Acetate + H₂O

First we calculate the number of moles of each reactant, using the given volumes and concentrations:

0.75 M Acetic acid * 50.0 mL = 37.5 mmol acetic acid

1.0 M NaOH * 10.0 mL = 10 mmol NaOH

We calculate how many acetic acid moles remain after the reaction:

37.5 mmol - 10 mmol = 27.5 mmol acetic acid

We now calculate the molar concentration of acetic acid after the reaction:

27.5 mmol / (50.0 mL + 10.0 mL) = 0.458 M

Then we calculate [H⁺], using the following formula for weak acid solutions:

[H⁺] = $\sqrt{C*Ka}=\sqrt{0.458M*1.76x10^{-5}}$

[H⁺] = 0.0028

Finally we calculate the pH:

pH = -log[H⁺]

pH = 2.66

8 0

2 years ago

Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coeff

ahrayia [7]

Answer:

NH4Br + AgNO3 —> AgBr + NH4NO3

Explanation:

When ammonium bromide and silver(I) nitrate react, the following are obtained as shown below:

NH4Br(aq) + AgNO3(aq) —>

In solution, NH4Br(aq) and AgNO3(aq) will dissociate as follow:

NH4Br(aq) —> NH4+(aq) + Br-(aq)

AgNO3(aq) —> Ag+(aq) + NO3-(aq)

The double displacement reaction will occur as follow:

NH4+(aq) + Br-(aq) + Ag+(aq) + NO3-(aq) —> Ag+(aq) + Br-(aq) + NH4+(aq) + NO3-(aq)

NH4Br(aq) + AgNO3(aq) —> AgBr(s) + NH4NO3(aq)

6 0

3 years ago