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makkiz [27]
2 years ago
11

What is (3 X 10^3) +(2.5 X 10^6)? *

Chemistry
2 answers:
DaniilM [7]2 years ago
5 0

Answer:

Scientific Notation: 2.503 × 10⁶

Standard Form: 2,503,000

Radda [10]2 years ago
3 0

Hey there!

\mathsf{(3 \times 10^3) + (2.5 \times 10^6)}

\mathsf{= 3 \times 10^3 + 2.5 \times10^6}

\mathsf{10^3}

\mathsf{= 10 \times 10 \times 10}

\mathsf{= 100 \times 10}

\mathsf{\bf = 1,000}

\mathsf{10^6}

\mathsf{= 10 \times 10 \times 10 \times 10 \times 10 \times 10}

\mathsf{= 100 \times100 \times100}

\mathsf{= 10,000\times100}

\mathsf{= \bf 1,000,000}

\mathsf{= 3\times 1,000 + 2.5 \times 1,000,000}

\mathsf{3\times1,000}

\mathsf{\bf = 3,000}

\mathsf{2.5 \times 1,000,000}

\mathsf{\bf = 2,500,000}

\mathsf{3,000 + 2,500,000}

\mathsf{= \bf 2,503,000}

\boxed{\boxed{\large\textsf{Answer: } \mathsf{ \bf 2,503,000 \ or \ 2.503 \times 10^6}}}\huge\checkmark

\large\textsf{Good luck on your assignment and enjoy your day!}

~\frak{Amphitrite1040:)}

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25cc of 5 % NaOH solution neutralized 30cc of h2sO4 solution. Whatis normality of H2SO4?
MAVERICK [17]

The normality of the H₂SO₄ that reacted with 25cc of 5 % NaOH solution is 1.1 N.

<h3>What is the molarity of 5% NaOH?</h3>

The molarity of 5% NaOH is 1.32 M

25 cc of NaOH neutralized 30cc of H₂SO₄ solution.

Equation of reaction is given below:

  • 2 NaOH + H₂SO₄ ---> Na₂SO₄ + 2 H₂O

Molarity of H₂SO₄ = 1.32 x 1 x 25/(30 x 2) = 0.55 M

  • Normality = Molarity × moles of H⁺ ions per mole of acid

moles of H⁺ ions per mole of H₂SO₄ = 2

Normality of H₂SO₄ = 0.55 x 2 = 1.1 N

In conclusion, the normality of an acid is determined from the molarity and the moles of H⁺ ions per mole of acid.

Learn more about normality at: brainly.com/question/22817773

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7 0
1 year ago
Calcium carbonate is often used as an antacid. Your stomach acid is composed of HCl at a pH of 1.5. If you ate toooo much Turkey
stiks02 [169]

<u>Answer:</u> 0.0237 g of calcium carbonate would be required to neutralize the given amount of HCl

<u>Explanation:</u>

pH is defined as the negative logarithm of hydrogen ion concentration present in the solution

pH=-\log [H^+]      .....(1)

Given value of pH = 1.5

Putting values in equation 1:

1.5=-\log[H^+]

[H^+]=10^{(-1.5)}=0.0316M

Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:

\text{Molarity of solution}=\frac{\text{Number of moles of solute}\times 1000}{\text{Volume of solution (mL)}}       .....(2)

We are given:

Volume of solution = 15.0 mL

Molarity of HCl = 0.0316 M

Putting values in equation 2:

0.0316=\frac{\text{Moles of HCl}\times 1000}{15.0}\\\\\text{Moles of HCl}=\frac{0.0316\times 15.0}{1000}=4.74\times 10^{-4}mol

The chemical equation for the reaction of HCl and calcium carbonate follows:

2HCl+CaCO_3\rightarrow H_2CO_3+CaCl_2

By the stoichiometry of the reaction:

2 moles of HCl reacts with 1 mole of calcium carbonate

So, 4.74\times 10^{-4}mol of HCl will react with = \frac{1}{2}\times 4.74\times 10^{-4}=2.37\times 10^{-4}mol of calcium carbonate

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of calcium carbonate = 2.37\times 10^{-4}mol

Molar mass of calcium carbonate = 100.01 g/mol

Putting values in the above equation:

\text{Mass of }CaCO_3=(2.37\times 10^{-4}mol)\times 100.01g/mol\\\\\text{Mass of }CaCO_3=0.0237g

Hence, 0.0237 g of calcium carbonate would be required to neutralize the given amount of HCl

7 0
2 years ago
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