A solution is made by mixing 1.5 g of Sr(OH) 2 and 23.5 mL of 1.000 M HNO 3 . (c) Is the resulting solution acidic or basic?

Calculate the number of moles of Sr(OH)_{2} by using its molar mass. The molar mass of Sr(OH)_{2} is calculated as follows: Sr = 87.62 g/mol, O = 16.00 g/mol, H = 1.01 g/mol. Thus, the molar mass of Sr(OH)_{2} = 87.62 + (16.00*2) + (1.01*2) = 121.64 g/mol. Use the formula: moles = mass / molar mass.. Calculate the number of moles of HNO_{3} using the concentration and volume. Convert the volume from mL to L by dividing by 1000. Then use the formula: moles = concentration (M) * volume (L).. Compare the moles of Sr(OH)_{2} and HNO_{3} to determine the limiting reactant. The reaction between Sr(OH)_{2} and HNO_{3} is a neutralization reaction, where Sr(OH)_{2} reacts with 2 moles of HNO_{3} for every mole of Sr(OH)_{2}.. Determine if there is any excess reactant. If there are more moles of Sr(OH)_{2} than required to completely react with the available moles of HNO_{3}, Sr(OH)_{2} is in excess and the solution will be basic. Conversely, if there are more moles of HNO_{3} than required to react with Sr(OH)_{2}, HNO_{3} is in excess and the solution will be acidic.. Conclude whether the solution is acidic or basic based on which reactant is in excess.

A solution is made by mixing 1.5 g of Sr(OH)2 and 23.5 mL of 1.000 M HNO3. (c) Is the resulting solution acidic or basic?

Calculate the number of moles of Sr(OH)_{2} by using its molar mass. The molar mass of Sr(OH)_{2} is calculated as follows: Sr = 87.62 g/mol, O = 16.00 g/mol, H = 1.01 g/mol. Thus, the molar mass of Sr(OH)_{2} = 87.62 + (16.00*2) + (1.01*2) = 121.64 g/mol. Use the formula: moles = mass / molar mass. Calculate the number of moles of HNO_{3} using the concentration and volume. Convert the volume from mL to L by dividing by 1000. Then use the formula: moles = concentration (M) * volume (L). Compare the moles of Sr(OH)_{2} and HNO_{3} to determine the limiting reactant. The reaction between Sr(OH)_{2} and HNO_{3} is a neutralization reaction, where Sr(OH)_{2} reacts with 2 moles of HNO_{3} for every mole of Sr(OH)_{2}. Determine if there is any excess reactant. If there are more moles of Sr(OH)_{2} than required to completely react with the available moles of HNO_{3}, Sr(OH)_{2} is in excess and the solution will be basic. Conversely, if there are more moles of HNO_{3} than required to react with Sr(OH)_{2}, HNO_{3} is in excess and the solution will be acidic. Conclude whether the solution is acidic or basic based on which reactant is in excess.

Ch.4 - Reactions in Aqueous Solution

Brown - Chemistry: The Central Science 14th Edition

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Ch.4 - Reactions in Aqueous Solution

Problema 88c

Capitolo 4, Problema 88c

A solution is made by mixing 1.5 g of Sr(OH)₂ and 23.5 mL of 1.000 M HNO₃. (c) Is the resulting solution acidic or basic?

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Calculate the number of moles of Sr(OH)₂ by using its molar mass. The molar mass of Sr(OH)₂ is calculated as follows: Sr = 87.62 g/mol, O = 16.00 g/mol, H = 1.01 g/mol. Thus, the molar mass of Sr(OH)₂ = 87.62 + (16.00*2) + (1.01*2) = 121.64 g/mol. Use the formula: moles = mass / molar mass.

Calculate the number of moles of HNO₃ using the concentration and volume. Convert the volume from mL to L by dividing by 1000. Then use the formula: moles = concentration (M) * volume (L).

Compare the moles of Sr(OH)₂ and HNO₃ to determine the limiting reactant. The reaction between Sr(OH)₂ and HNO₃ is a neutralization reaction, where Sr(OH)₂ reacts with 2 moles of HNO₃ for every mole of Sr(OH)₂.

Determine if there is any excess reactant. If there are more moles of Sr(OH)₂ than required to completely react with the available moles of HNO₃, Sr(OH)₂ is in excess and the solution will be basic. Conversely, if there are more moles of HNO₃ than required to react with Sr(OH)₂, HNO₃ is in excess and the solution will be acidic.

Conclude whether the solution is acidic or basic based on which reactant is in excess.

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Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, Sr(OH)2 is a strong base that dissociates in solution to produce hydroxide ions (OH-), while HNO3 is a strong acid that dissociates to produce hydrogen ions (H+). The resulting pH of the solution will depend on the relative amounts of acid and base present.

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Percorso guidato

01:09

Acid-Base Reaction

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. To determine whether the solution is acidic or basic, one must calculate the moles of Sr(OH)2 and HNO3. This involves converting grams of Sr(OH)2 to moles and using the molarity of HNO3 to find its moles, allowing for a comparison of the acid and base present in the solution.

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Percorso guidato

01:16

Stoichiometry Concept

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral. A solution is considered acidic if its pH is less than 7 and basic if its pH is greater than 7. After determining the moles of acid and base, the resulting pH can be calculated to classify the solution accordingly.

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02:33

The pH Scale

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