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Vladimir79 [104]
3 years ago
15

Part A Which acid in each of the following pairs has the stronger conjugate base? Match the words in the left column to the appr

opriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. ResetHelp Of the acids HCl or HF, the one with the stronger conjugate base is Of the acids H C l or H F, the one with the stronger conjugate base is blank.. Of the acids H2S or HNO2 , the one with the stronger conjugate base is Of the acids H 2 S or H N O 2 , the one with the stronger conjugate base is blank.. Of the acids H2CO3 or HClO4 , the one with the stronger conjugate base is Of the acids H 2 C O 3 or H C l O 4 , the one with the stronger conjugate base is blank.. Of the acids HF or NH4+, the one with the stronger conjugate base is Of the acids H F or N H 4 +, the one with the stronger conjugate base is blank..
Chemistry
1 answer:
vichka [17]3 years ago
6 0

Answer:

HF

H₂S

H₂CO₃

NH₄⁺

Explanation:

<em>Which acid in each of the following pairs has the stronger conjugate base?</em>

According to Bronsted-Lowry acid-base theory, <em>the weaker an acid, the stronger its conjugate acid</em>. Especially for weak acids, pKa gives information about the strength of such acid. <em>The higher the pKa, the weaker the acid.</em>

<em />

  • Of the acids HCl or HF, the one with the stronger conjugate base is HF because it is a weak acid.
  • Of the acids H₂S or HNO₂, the one with the stronger conjugate base is    H₂S  because it is a weaker acid. pKa (H₂S) = 7.04 > pKa (HNO₂) = 3.39
  • Of the acids H₂CO₃ or HClO₄, the one with the stronger conjugate base is H₂CO₃ because it is a weak acid.
  • Of the acids HF or NH₄⁺, the one with the stronger conjugate base is NH₄⁺ because it is a weaker acid. pKa (HF) = 3.17 < pKa (NH₄⁺) = 9.25
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The mass of Ba(IO3)2 that can be dissolved in 500 ml of water at 25 degrees celcius is 2.82 g

<h3>What mass of Ba(IO3)2 can be dissolved in 500 ml of water at 25 degrees celcius?</h3>

The Ksp of Ba(IO3)2 = 1.57 × 10^-9

Molar mass of Ba(IO3)2 = 487 g/mol?

Dissociation of Ba(IO3)2 produces 3 moles of ions as follows:

Ba(IO_{3})_{2} \leftrightharpoons Ba^{2+} + 2\:IO_{3}^{-}

Ksp = [Ba^{2+}]*[IO_{3}^{-}]^{2}

[Ba(IO_{3})_{2}] =  \sqrt[3]{ksp} =\sqrt[3]{1.57 \times  {10}^{ - 9} } \\  [Ba(IO_{3})_{2}] = 1.16 \times  {10}^{-3} moldm^{-3}

moles of Ba(IO3)2 = 1.16 × 10^-3 × 0.5 = 0.58 × 10^-3 moles

mass of Ba(IO3)2 = 0.58 × 10^-3 moles × 487 = 2.82 g

Therefore, mass Ba(IO3)2 that can be dissolved in 500 ml of water at 25 degrees celcius is 2.82 g.

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Use the reaction given below to solve the problem that follows: Calculate the mass in grams of aluminum oxide produced by the re
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Thus 0.556 moles of Al will produce=\frac{2}{4}\times 0.556=0.278moles  of Al_2O_3

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