# Acid Base Titration Problems, Basic Introduction, Calculations, Examples, Solution Stoichiometry

TLDRThis educational video script offers a comprehensive guide on solving acid-base titration problems using two primary methods: equations and stoichiometry. It demonstrates the process of neutralization reactions involving monoprotic acids and bases, utilizing the formula m1v1 = m2v2 to find the concentration of acids like HCl and bases like NaOH. The script also covers the calculation of volumes required for neutralization using balanced chemical equations and molar ratios, exemplified with reactions involving barium hydroxide and nitric acid, as well as potassium hydrogen phthalate and sodium hydroxide. The step-by-step approach simplifies complex titration concepts, making it accessible for students and learners in chemistry.

###### Takeaways

- ๐งช The video focuses on solving acid-base titration problems using two methods: equations and dimensional analysis.
- ๐ The first example involves neutralizing 24.7 mL of HCl solution with 35.8 mL of 0.25 M NaOH solution, aiming to find the concentration of the original HCl solution.
- ๐ For monoprotic acids and bases, the formula m1v1 = m2v2 is used, where m is molarity and v is volume, to find the moles of acid and base involved in the reaction.
- โ๏ธ The concentration of HCl is calculated to be 0.362 M using both the equation method and dimensional analysis, confirming the consistency of the two approaches.
- ๐ The second problem involves finding the volume of 0.15 M barium hydroxide solution needed to neutralize 45 mL of 0.29 M HNO3 solution, considering the stoichiometry of the reaction.
- ๐ The balanced chemical equation for the reaction between barium hydroxide and nitric acid shows a one-to-two molar ratio, which is crucial for calculating the required volume.
- ๐ The volume of barium hydroxide solution required is calculated to be 43.5 mL, using both the modified equation method and stoichiometry.
- ๐งช The third problem asks for the mass of KHP that will be completely neutralized by 32.57 mL of a 0.175 M sodium hydroxide solution, using stoichiometry due to the mass being involved.
- โ๏ธ The molar mass of KHP is used to convert grams to moles, and the one-to-one molar ratio between KHP and NaOH is applied to find the mass of KHP to be 1.164 grams.
- ๐ The fourth problem calculates the concentration of KOH solution used to titrate 0.137 grams of KHP, again using a one-to-one molar ratio and the molar mass of KHP.
- ๐ The concentration of KOH is determined to be 0.01 M, found by dividing the moles of KOH by the volume of the solution in liters.

###### Q & A

### What is the main topic of the video?

-The main topic of the video is solving acid-base titration problems.

### How many methods are discussed in the video to solve the first titration problem?

-Two methods are discussed in the video to solve the first titration problem: using an equation and by dimensional analysis.

### What is the formula used in the first method to find the concentration of the original HCl solution?

-The formula used in the first method is m1v1 = m2v2, where m1 and v1 correspond to the acid, and m2 and v2 correspond to the base.

### What is the balanced chemical equation for the reaction between HCl and sodium hydroxide?

-The balanced chemical equation is HCl + NaOH โ NaCl + H2O, indicating a double replacement reaction.

### What is the concentration of the original HCl solution calculated in the video?

-The concentration of the original HCl solution is calculated to be 0.362 moles per liter.

### How does the video approach the problem involving barium hydroxide and nitric acid?

-The video approaches the problem by modifying the equation m1v1 = m2v2 to account for the two hydroxide ions in barium hydroxide and then solving for the volume of barium hydroxide solution required.

### What is the volume of barium hydroxide solution required to neutralize the given nitric acid solution in the third problem?

-The volume of barium hydroxide solution required to neutralize the given nitric acid solution is 43.5 milliliters.

### How does the video solve the problem involving potassium hydrogen phthalate (KHP) and sodium hydroxide (NaOH)?

-The video solves the problem by using stoichiometry, starting with the moles of NaOH, converting it to moles of KHP, and then using the molar mass of KHP to find the mass in grams.

### What mass of KHP is completely neutralized by 32.57 milliliters of a 0.175 molar standard sodium hydroxide solution according to the video?

-The mass of KHP that is completely neutralized is 1.164 grams.

### In the final problem, what is the concentration of the KOH solution used to titrate KHP?

-The concentration of the KOH solution used to titrate KHP is 0.01 moles per liter.

###### Outlines

##### ๐งช Solving Acid-Base Titration Problems

This paragraph introduces the topic of solving acid-base titration problems using two methods: an equation and dimensional analysis. It presents a specific problem involving the neutralization of an HCl solution by a sodium hydroxide solution. The monoprotic nature of the acid and base allows for a straightforward calculation using the formula m1v1 = m2v2, where m is molarity and v is volume. The example calculates the concentration of the original HCl solution to be 0.362 moles per liter.

##### ๐ Neutralizing Barium Hydroxide with Nitric Acid

The second paragraph discusses the titration of a barium hydroxide solution with a nitric acid solution. It highlights the need to adjust the equation due to barium hydroxide having two hydroxide ions per formula unit. The stoichiometry of the reaction is used to calculate the volume of barium hydroxide required to neutralize the nitric acid. The balanced chemical equation Ba(OH)2 + 2HNO3 โ Ba(NO3)2 + 2H2O is used to determine the molar ratio, leading to the calculation of 43.5 milliliters of barium hydroxide needed for neutralization.

##### ๐งช Determining the Mass of KHP Neutralized by Sodium Hydroxide

This paragraph focuses on the neutralization of potassium hydrogen phthalate (KHP) by a standard sodium hydroxide solution. It emphasizes that stoichiometry is the best method for this problem due to the need to relate moles to mass. The balanced chemical equation KHP + NaOH โ NaKP + H2O is used to establish a one-to-one molar ratio. The moles of NaOH are calculated from its concentration and volume, then used to find the moles of KHP. Finally, the molar mass of KHP is applied to determine the mass of KHP that will be completely neutralized, which is found to be 1.164 grams.

##### ๐ Calculating KOH Solution Concentration from KHP Titration

The final paragraph explains how to find the concentration of a KOH solution using the titration with KHP. It starts with the given mass of KHP and converts it to moles using the molar mass of KHP. The one-to-one molar ratio between KHP and KOH is used to find the moles of KOH. The concentration of KOH is then calculated by dividing the moles of KOH by the volume of the solution in liters. The calculated concentration of the KOH solution is 0.01 moles per liter.

###### Mindmap

###### Keywords

##### ๐กAcid-Base Titration

##### ๐กMolarity

##### ๐กMonoprotic Acid

##### ๐กNeutralization Reaction

##### ๐กStoichiometry

##### ๐กBalanced Chemical Equation

##### ๐กMolar Ratio

##### ๐กMoles

##### ๐กVolume Conversion

##### ๐กMolar Mass

###### Highlights

The video focuses on solving acid-base titration problems using two methods: an equation and dimensional analysis.

A monoprotic acid and base with one hydrogen and hydroxide ion per formula unit can be solved using the formula m1v1 = m2v2.

The molarity of the original HCl solution is calculated to be 0.362 moles per liter.

Dimensional analysis is a simple method for solving titration problems with monoprotic acid and base.

A balanced chemical equation is essential for stoichiometry in titration problems.

The molar ratio in a balanced chemical equation is crucial for determining the volume of barium hydroxide solution required.

The volume of barium hydroxide solution needed to neutralize nitric acid is calculated to be 43.5 milliliters.

For titration involving a monoprotic acid like KHP, stoichiometry is the preferred method over the m1v1 = m2v2 formula.

The mass of KHP neutralized by sodium hydroxide is determined to be 1.164 grams.

A one-to-one molar ratio is observed between KHP and sodium hydroxide in the balanced chemical reaction.

The concentration of KOH solution is calculated using the mass of KHP and the volume of KOH solution.

The concentration of KOH is found to be 0.01 moles per liter.

Understanding the molar mass of KHP is key to converting moles to grams in titration calculations.

The video demonstrates the importance of matching units when performing titration calculations.

The video provides step-by-step instructions for solving titration problems, enhancing clarity and understanding.

The video concludes with a summary of the methods used to find the concentration of KOH and the mass of KHP.

###### Transcripts

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