**Table 1: Standardization Data**| | Trial 1 | Trial 2 ||--------------------|-----------|----------|| **Mass of KHP** | 0.4550 g | 0.4536 g || **Initial burette reading** | 12.75 mL | 12.8 mL || **Final burette reading** | 28.0 mL | 26.0 mL || **Volume of base used** | 15.25 mL | 13.2 mL |---**Data Analysis:**1. **Calculate the molarity of base (for each trial).** You must use dimensional analysis—show all unit conversions (hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Experiment 11, Part 1.**Trial 1:**- $0.4550 \, \text{g KHP}$**Trial 2:**\[Molarity: \frac{\text{grams of KHP}}{\text{volume of base (L)} \times \text{molar mass of KHP}}\]---**Average:**1. Calculate the average molarity from both trials.---Instructions for the calculations involve using the relationship between moles, volume, and molarity, specifically using the mass of KHP (Potassium hydrogen phthalate) to find the concentration of the base in the titration experiments.

To calculate the Molarity of base, we would first check the mole ratio between base and KHP from the…

M: Table 1: Standardization Data Trial 1 Trial 2 Mass of KHP O145504 0.05ML 04536 12.3 mL Initial burette reading Final burette reading 12.8 a6.omL Volume of base used 12.75 13.2 mL Data Analysis: KH Cg Hg Da GHOIAR MASS 20412) 1. Calculate the molarity of base for each trial. You must use dimensional analysis - show all unit conversions (hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Expt 11 part 1.

M: Table 1: Standardization Data Trial 1 Trial 2 Mass of KHP O145504 0.05ML 04536 12.3 mL Initial burette reading Final burette reading 12.8 a6.omL Volume of base used 12.75 13.2 mL Data Analysis: KH Cg Hg Da GHOIAR MASS 20412) 1. Calculate the molarity of base for each trial. You must use dimensional analysis - show all unit conversions (hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Expt 11 part 1.

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...

See similar textbooks

Similar questions

> EL session.masteringchemistry.com MasteringChemistry ROSTER-2019-SPRI-PULLM-CHEM-101 blackboard wsu Google Search MasteringChemistry: HW 8 KHW 8 Applications for Dilution Calculations K8 of8 Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations wavelengths in the visible (and sometimes uitraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. reach the dete ctor, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque…
Given the following data Dissolved Oxygen Titration Data Trial 1 Preparation of titrant 0.4455 g NazS203•5H20 in 50.0 mL water Mass of water sample used (g) 5.21 g Initial mass of Na2S203 soln and Beral pipet(g) 12.40 g Final mass of Na2S203 soln and Beral pipet(g) 12.20 g MW of Na2S203•5H2O 248.11 g/mol MW of NazS203 158.11 g/mol MW of O2 32 g/mol Calculate the following: a) Concentration of Na2S203•5H20 in mol/g c) DO of sample (ppm) Final answer: 3 significant figures
Cc.1.
Exercise 14.72 - Enhanced - with Feedback MISSED THIS? Watch KCV: Solution Concentration: Molarity, Molality, Parts by Mass and Volume, Mole Fraction, IWE: Converting between Concentration Units; Read Section 14.5. You can click on the Review link to access the section in your e Text. One brand of laundry bleach is an aqueous solution containing 4.00% sodium hypochlorite (NaOCI) by mass. < Previous OL ASU
[Review Topics] [References) entration TUTOR Determining Mole Fraction and Mass Percent An aqueous solution of ethanol, CH,CH,OH, has a concentration of 6.99 mol/L and has a density of 0.947 g/mL. What are the mass percent and mole firaction of CHCH,OH in this solution? Mass percent CH3CH,OH = Mole fraction CH CH,OH = Submit Show Approach Show Tutor Steps progress Retry Entire Group 8 more group attempts remaining mit Answer Previous Next Email Instructor Save and Ex (? 72"F Cloudy 9:58 A 9/10/2 40 144 40A prt sc delete home end 80 %3D backspace num lock 7. home enter
Please give me both right solutions.. urgenttttttttt
FSC 8 1921. Brightspace A Aktiv Chemistry C D Z < Q + # At F2 @ 2 What volume in mL of 0.3000 M NaCl solution is required to produce 0.2700 moles of NaCl? W S app.101edu.co Walmart - Hiring Ce... X F3 X # 3 11. Unit 12: Late Adulthood - Develo X E JC 4 D F4 с 144 $ JU F5 R LL F ► 11 % 5 V F6 t 44 T G A 6 F7 Simulation play - Labster B Y H F8 & 7 8 U N Question 7 of 9 DELL F9 X D * 8 J F10 ( M Walmart - Hiring Center 9 F11 JI K 2 O ) O F12 L P 4 : 7 +/- PrtScr W 8 Insert { ( **
In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9 How many millimoles of Ba(NO3)2 are there in the solution? Hide answer choices 250 mmol 125 mmol 50 mmol 25 mmol
If you use [KMnO4]=0.0252 M, Concentration of FeSO4 7 H2O = 5.70 g/L Using a 100-mL graduated cylinder, 50 mL sample of FeSO4*7 H₂O will be measured out. To each sample of FeSO4 7 H2O, add 10.0 mL of H2SO4 and 10 mL of H3PO4 Concentration of SnCl2 2 H2O 2.85 g/mL Using a 100-mL graduated cylinder, 50.0 mL sample of SnCl2 2 H₂O will be measured out. No additional acid is needed. #1 KMnO4 #1 KMnO4 Sample # Initial buret, mL Final buret, mL FeSO4*7 H2O 12.05 21.51 SnCl2 2 H₂O 0.07 9.54 Question) Answer the following questions. b) Determine mol of electron lost per mol of Sn ion. 1) In this case, your answer should be in decimal notation (for example, 0.123, not 1.23*10^-1) with the correct number of significant figures. Also follow the unit specified in each question. Do NOT put its unit in your answer because its unit is shown already in the questions.
K2CO3 (aq)+ CaCl2 (aq)→ CaCO3 (s) + 2KCl (aq) Data Sheet Table 1: Data and Observations Material Mass CaCl2 2.0g K2CO3 2.5g Filter Paper 1.6g Watch Glass 35.8g Filter Paper + Watch Glass + Precipitate 38.9 Precipitate 1.5g Table 2: Mass of CaCl2 after 24 Hours Initial Observations 24 hour Observation Weigh Boat Mass of Weigh Boat 0.5g Mass of Weigh Boat 0.5g CaCl2 2.0g Mass of CaCl2 2.4g Mass of CaCl2 Calculate the theoretical yield of the solid precipitate. Then use that to calculate the percent yield of the solid precipitate.
answer number 9. show your solutions
How do you find weight of Na2C2O4 in unknown?