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 HNO 3 . (c) Is the resulting solution acidic or basic?

Hi everyone here, we have a question asking is the following solution acidic or basic. And it tells us that a solution is made by mixing 2.43 g of acetic acid, ch three C 00 H and 25.0 mL of 1.43 moller sodium hydroxide solution. So first we need to find the moles of each. So we'll start off with acetic acid And it has 2.43 g. We're going to multiply that by one mole Divided by its Molar Mass, which is 60.05. Our g here are going to cancel out, leaving us with zero 0. 05 moles. And now we're going to do the same with sodium hydroxide. But sodium hydroxide, we have milliliters and molar charity. So we're going to start off with our 25.0 ml. And we're going to first change that to leaders. So 10 to the negative. Three leaders over one millimeter Times 1.43 moles over one liter. Because polarity is moles over leader. So our middle leaders are canceling out here and our leaders are canceling out here And that leaves us with 0. 358 moles. Now let's write out the reaction we have. So we have acetic acid plus sodium hydroxide forming sodium acetate and water. So this is already balanced. So our multiple ratio is 1-1. So we have one mole of sodium hydroxide reacting with one mole of acetic acid. So the moles of acetic acid is greater than the moles, sodium hydroxide, meaning that it is the accessory agent and therefore the solution will be acidic. And that is our final answer. Thank you for watching. Bye.

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

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 88c

Chapter 4, Problem 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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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.

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.