Titration lab: NaOH +HCl->NaCl+H2O • Watch the video : htps:/www.youtube.com/watch?v=cdvkZCNhvf4 • Initial volume of NaOH in the burete= 0.90ml • Final volume of NaOH in the burete=30.90 • Volume of NaOH= final volume-initial volume=30.0 ml NaOH • M NAOH= 0.10M > 0. ImolL. NaOH • FIRST TITRATION=is to find the exact Mof N2OH WE Call the first experiment= standardization of base • We found out the Mof base =0.10 M • Volume of HCl in the flask= 10.00 ml they grabbed it with pipet glassware. Pipette is reaaly precise even more than graduated cylinder we should go upto two after decimal point. • M of HC? Chapter 7 flash back 30.0ml N2OHX IL NAOH x 0.10molNaOH xImol HCI = 0.003mol HCI 1000ml NaOH IL NaOH Imol NaOH Find M of HCI?

Titration lab: NaOH +HCl->NaCl+H2O • Watch the video : htps:/www.youtube.com/watch?v=cdvkZCNhvf4 • Initial volume of NaOH in the burete= 0.90ml • Final volume of NaOH in the burete=30.90 • Volume of NaOH= final volume-initial volume=30.0 ml NaOH • M NAOH= 0.10M > 0. ImolL. NaOH • FIRST TITRATION=is to find the exact Mof N2OH WE Call the first experiment= standardization of base • We found out the Mof base =0.10 M • Volume of HCl in the flask= 10.00 ml they grabbed it with pipet glassware. Pipette is reaaly precise even more than graduated cylinder we should go upto two after decimal point. • M of HC? Chapter 7 flash back 30.0ml N2OHX IL NAOH x 0.10molNaOH xImol HCI = 0.003mol HCI 1000ml NaOH IL NaOH Imol NaOH Find M of HCI?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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EXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155
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MISSED THIS? Watch IWE 14.4; Read Section 14.6. You can click on the Review link to access the section in your e Text. Four solutions of unknown NaOH concentration are titrated with solutions of HC1. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. NaOH volume (mL) 6.00 22.00 14.00 28.00 HCl volume [HC1] (mL) (M) 7.97 0.1799 11.24 10.95 33.18 0.1311 0.0789 0.1421 Part C Calculate the concentration (in M) of the unknown NaOH solution in the third case. NaOH volume (mL) HCl volume (mL) [HC1] (M) 14.00 10.95 0.0789 Express your answer using three significant figures. concentration = Submit Part D 15 ΑΣΦ Request Answer ? Express your answer using four significant figures. P Pearson Review | Constants | Periodic Table M Calculate the concentration (in M) of the unknown NaOH solution in the fourth case. NaOH volume (mL) HCl volume (mL) 28.00 33.18 [HC1] (M)…
A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. The Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Kb, set up the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. [0] [0.200 + x] [0.175 + x] [0.200] [0.200 -x] [0.175 -x] 0 1.70 Kb 4.77 x 10-1⁰ = 12.3 [0.0200] [0.100] [0.0200 + x] [0.0200 -x] 10.8 [0.140] 2 [0.100 + x] 2.10 x 10-² A student was titrating a solution of hydrazine (H₂NNH₂) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the…
help with part b please