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Lera25 [3.4K]
2 years ago
6

Whose power in the Senate is equal to the power of the Speaker of the House? Senate Chief of Staff President of the Senate Senat

e Majority Leader Senate Majority Whip
SAT
2 answers:
Sophie [7]2 years ago
6 0

The power of the Majority leader in the Senate is equal to the power of the Speaker of the House

for better understanding let's explain who majority leader means

  • Majority Leader is known to be a floor leader of the party that holds the majority of seats in each house of Congress.

  • Speaker of the House is simply known to one of the more powerful and important people within the halls of Congress. This position is are often both elected and is the presiding officer of the House and the known leader of its majority party

from the above we can therefore say that the answer The power of the Majority leader in the Senate is equal to the power of the Speaker of the Houses is correct

learn more about majority leader from:

brainly.com/question/2070369

BlackZzzverrR [31]2 years ago
5 0

Answer:

<h2>C.) Senate Majority Leader</h2>

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A 20.0-ml sample of a 0.200 mhbr solution is titrated with a 0.200 mnaoh solution. calculate the ph of the solution after the fo
kumpel [21]

The calculated pH of the solutions are given below:

  • The pH of the solution after 14.0 ml of base is added to it is calculated as 1.45.
  • The pH of the solution after 19.8 ml of base is added to it is calculated as 3.0
  • The pH of the solution after 20.0 ml of base is added to it is calculated as 7.

<h3>What is pH?</h3>

This is the level of acidity or alkalinity of an aqueous solution. The pH of a substances tells if its an acid, base or neutral.

HBr and NaOH while in water would dissociate and they would become H+ and OH- respectively.

Mol of HBr = Mol * Vol

= 0.200 * 20mL

= 4 mmol

A. Moles of NaOH added

= 0.2 X 14

= 2.8 mmol

Moles of H+ that did not react

= 4 - 2.8

= 1.2 mmol

1.2/1000 = 0.0012 moles

Total volume = 20 + 14

= 34 mL to litres

= 0.034 L

Molarity of H+ = 0.0012 / 0.034L

= 0.035 M

-log[0.035] = 1.45

The pH of the solution is  1.45

B. NaOH added = 19.8 * 0.2 =

3.96 mmoles

The unreacted solution

= 4.0 - 3.96

= 0.04 mmol

0.04/1000 = 0.00004 moles

Total volume = 20 + 19.8

= 39.8mL

Converted to litres = 0.0398L

Molarity  = 0.00004 / 0.0398L

= 0.001

-log(0.001) = 3.0

The ph Is therefore 3.0

C. Moles of NaOH added = 0.2*20mL = 4mmol

All the H+ are going to be consumed here. This would result into a neutral solution pH = 7

<u>Complete question:</u>

20.0 mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the PH of the solution after the following volumes of base have been added.

A. 14.0 mL

B. 19.8 mL

C. 20.0 mL

Read more on pH here; brainly.com/question/22390063

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