measured by molarity (M), which is the number of moles per liter of solution (moles/L). For example,1 M = 1 mole/L. To determine how many grams of a substance is equal to one mole the molecularmass is needed (we will not explore this in this lab rather this is taught in your Chemistry subjects).The general formula for making a dilution solution is the following:CaV1 = C2V2whereC1 = the original concentration of stock solutionVi = the volume of stock solution needed to make working solutionC2 = the desired concentration of working solutionV2 = the desired final volume of working solutionHow would you make a 100 ul working stock at a concentration of 0.5 uM from a stock solutionat a concentration of 0.1 mM? Always remember to put everything into the same units first!For Educational Purposes OnlySLSU-TO/NCMatondoWhat would be the working stock concentration (in molarity) if you diluted 250 µl of a stockconcentration of 10 uM in a total volume of 1 ml?LAB EXERCISE NO. 4. PATTERN OF INHERITANCEn (] II

Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

V2 = the desired final volume of working solution How would you make a 100 ul working stock at a concentration of 0.5 uM from a stock solution at a concentration of 0.1 mM? Always remember to put everything into the same units first!

V2 = the desired final volume of working solution How would you make a 100 ul working stock at a concentration of 0.5 uM from a stock solution at a concentration of 0.1 mM? Always remember to put everything into the same units first!

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

What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 MNAOH? |g Fe(OH)3
A. How many mL of a 0.171 M aqueous solution of nickel(II) nitrate, Ni(NO3)2, must be taken to obtain 13.1 grams of the salt? B. How many milliliters of 9.95 M hydrochloric acid solution should be used to prepare 4.00 L of 0.300 M HCl? C. Calculate the number of milliters of 0.764 M NaOH required to precipitate as AgOH all of the Ag+ ions in 167 mL of 0.632M AgNO3 solution. D. An aqueous solution of hydrobromic acid is standardized by titration with a 0.169 M solution of barium hydroxide.If 13.0 mL of base are required to neutralize 13.0 mL of the acid, what is the molarity of the hydrobromic acid solution? E. Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is H2C2O4•2H2O.A student dissolves 0.631 grams of H2C2O4•2H2O in water and titrates the resulting solution with a solution of sodium hydroxide of unknown concentration. If 24.1 mL of the sodium hydroxide solution are required to neutralize the acid, what is the…
8. How many grams and moles of solute are there in 250. mL of a 0.1OM CaCl, solution?
Write a step-by-step prodcedure how how to create 100.0 mL of a 0.024 M solution of potassium iodate from a 0.048 M solution of potassium iodate (pretend you are creating this procedure for someone unfamiliar to chemistry and making solutions; be specific in your procedure and show your calculations)
A sample of potassium bicarbonate (KHCO3) was reacted with HCl to produce KCl. The following data was collected. Mass of beaker 28.43 g Mass of beaker + KHCO3 36.95 g Volume of HCl 12.0 mL Concentration of HCl 9.0 M Mass of beaker +residue (KCl) 33.82 g Calculate the following quantities. Show calculations where requested: Mass of KHCO3 __________________ Mass of residue __________________ Mass of 1 mol of KHCO3 __________________ No. of moles of KHCO3 used ___________________ Show calculations below No. of moles of HCl added ____________________ Show calculations below: Assuming KHCO3 is the limiting reactant, how many grams of KCl can be formed? Show calculations below: Assuming HCl is the limiting reactant, how many grams of KCl can be formed? Show calculations below: Which reactant is limiting? ___________________ Which reactant is excess? ____________________ Actual yield of KCl: ______________________ Theoretical yield of KCl: ______________________ Percent yield of KCl:…
I'm a bit confused with this one. thank you
6. A 0.4622-g sample of potassium hyd rogen phthalate was dissolved in 50 mL of deionized water and titrated to a phenolphthalein end-point with 19.48 mL of NaOH solution. What is the molarity of the NaOH? 7. Assuming that the density of vinegar is 1.012 g/m L, calculate the weight percent of acetic acid in vinegar if 23.85 mL of 0.1311 M NaOH was required to titrate 5.00 mL of vinegar. did HA nd dis 192 riw o asuuc no'noleauoetb s obulbo. As 900 900 4Coz2 anigll .asbtucf namheqx dini 209 (0 HoO Cag) (es) ibis 9C D DV 9 ballet tnabole A 9 u u 1oied qütenud orlf hi asiddud e 9t borsoog szib alddud sis ord nolt dsvawnlcrndtuodA 9l il blucwnolduloe HOe wans uoy nistqx3 Sipid oo! tstse : wot oo dhelom t bbs rg beau yilednobbos nsbile s est itbin ow osta isrl bsbne evicmi Srtulce HOs orts to yahelom orld ininetsb as 9 adant anoto toi n odslo 613 Exbiont Aorf
Please use dimensional analysis to answer these
If 0.500 mL of an 0.219 M NaCl solution is added to 100.0 mL of pure water. what is the concentration of the new solution? Your answer should have 3 sig figs
esc Fr 2 What mass of precipitate is formed when 100. mL of 0.300 M NaCl reacts with 100. mL of 0.150 M Pb(NO3)? Round your answer to 3 significant digits. 55°F Clear 1 F1 B.D F2 @ 2 F3 3 E F4 LA 4 x10 Q Search F5 X % 5 S F6 C A 6 F7 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibil B 8 & 7 F8 * ос F9 DELL prt sc F10 home Submit Assignment F11 A end F12 insert + 5/
If 0.500 mL of an 0.208 M NaCl solution is added to 100.0 mL of pure water. what is the concentration of the new solution? Your answer should have 3 sig figs
1. What is the mass of the solution when 50.0 mL of 1.0 M HCI solution is mixed with 50.0 mL of 1.0 M NaOH solution? (d = 1.02 g/mL )