The following tabulated data is provided to answer this question and the remaining questions in the quiz. The post lab data will appear each page so that you can refer back to this data, as needed. Review the data, then answer the first question below. The equation is H2SO4 + NaOH → Na2SO4 + H2O (note, this equation is unbalanced) The last two rows are left blank because they will be filled in by your calculations. Titration Lab Trial 1 Trial 2 Trial 3 Volume of Acid Used 20.0 mL 20.2 mL 20.8 mL Molarity of Acid Used 0.05 M 0.05 M 0.05 M Initial Buret Reading 0.00 mL 0.00 mL 0.00 mL Final Buret Reading 20.7 mL 21.0 mL 21.5 mL Volume of NaOH Used Molarity of NaOH Solution What is the correct balanced equation for the neutralization reaction? Select one: a. H2SO4 + NaOH → Na2SO4 + H2O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 d. H2SO4 + 2 NaOH → Na2SO4 + 2 H20

The following tabulated data is provided to answer this question and the remaining questions in the quiz. The post lab data will appear each page so that you can refer back to this data, as needed. Review the data, then answer the first question below. The equation is H2SO4 + NaOH → Na2SO4 + H2O (note, this equation is unbalanced) The last two rows are left blank because they will be filled in by your calculations. Titration Lab Trial 1 Trial 2 Trial 3 Volume of Acid Used 20.0 mL 20.2 mL 20.8 mL Molarity of Acid Used 0.05 M 0.05 M 0.05 M Initial Buret Reading 0.00 mL 0.00 mL 0.00 mL Final Buret Reading 20.7 mL 21.0 mL 21.5 mL Volume of NaOH Used Molarity of NaOH Solution What is the correct balanced equation for the neutralization reaction? Select one: a. H2SO4 + NaOH → Na2SO4 + H2O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 d. H2SO4 + 2 NaOH → Na2SO4 + 2 H20

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 91A

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In an experiment to determine the amount of aspirin in a tablet, one of the bottles of NaOH used was accidentally left open for 24 hours, which lead to it reacting with carbon dioxide. What will be the effect on the calculated amount of aspirin compared to the actual amount in the tablet and the concentration of the NaOH solution? Calculated amount increases since NaOH concentration will be lower than original. Calculated amount increases since NaOH concentration will be higher than original. Calculated amount decreases since NaOH concentration will be lower than original. Calculated amount decreases since NaOH concentration will be higher than original.
Why does Cl- will increase if you add HCl in the reaction? Please explain briefly
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First read the text sections 10.5 and 10.6 on pH. This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power H+ Molarity X OH- Molarity), www we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10…
(References] This question has multiple parts. Work all the parts to get the most points. Use the References to access important values if needed for this question. The [OH ] of a solution can be determined from the pOH using the equation: [OH] = 10-POH Where: [OH]= hydroxide ion concentration a Use the rules for logarithms and exponents to solve for pOH in terms of [OH ]. NOTE: Capitalization counts. pOH= Submit Submit Answer Retry Entire Group 4 more group attempts remaining Previous Next
First read the text sections 10.5 and 10.6 on pH. This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to…
Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml…
Here is ph of the molarity of butyl chloride (C,H,CI) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. у 0.030- 0.0247 olo 0.020- Ar M 0.015- 0.010- 0.005- 500 1000 1500 2000 2500 3000 seconds created x10 Is C,H,Cl being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If C,H,Cl is being created or destroyed, what is the rate at which it is being created or destroyed 1200 seconds after the reaction starts? Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
Can you please tell me what's the classify reaction for NaOH(aq)+HCI(aq). I've attached two images here. The one is for the record data and the other one is the test tube where we have to look for the reaction and then record data in our lab.
Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answer
Which product contains a strong base that would most likely completely dissolve in water? O drain cleaner ammonia baking soda antacid Next Save and Exit Mark this and return .com/ContentViewers/AssessmentViewer/Activit.
Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?