How many grams of pure Na2CO3 are weighed and dissolved in a solution if you are to prepare a o.5320 N of HCI that utilized 48.12 ml of titrant? (MW`of Na2CO3 = 106 g/mol) Na2CO3+ H20 <=> 2NAOH + H2CO3 Type only the numerieal value in three significant figures.
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- What is the concentration of a standardized HCl solution that required 50.78 mL of HCl to titrate 0.7682 g of a primary standard Na2CO3? Na2CO3 + 2HCl --> H2CO3 + 2NaCl Na2CO3 = 105.99 g/mol ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS.3:59 PM Wed Mar 15 ... ap here or pull up for additional resources Question 74 of 75 A 25.0 mL solution of HNO3 is neutralized with 16.5 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO3 solution? 1 4 7 +/- 1 M 2 3 5 6 8 9 O LTE 32% Submit XC с x 100UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
- Help )) 32% Mon 1:12 AM dix-d.pdf AC=8935a868521ec4cdala6e89069b89458#10001 6 o I Review I Constants I Periodic Table Calculate the concentration of CIO, at equilibrium if the initial concentration of HCIO2 is 2.17x10-2 M. Express the molarity to three significant digits. 响 AX中 [CIO2 | = M Submit Request Answer Part C Calculate tm concentration of HC1O2 at equilibrium if the initial concentration of HC1O2 is 2.17x10-2 M . Express the molarity to three significant digits. ? [HCIO2] = P Pearson Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy Permissions | Contact Us | 895 102 W tv MacBook Air 圓 國o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remainingExp. 4 Volhard method In an experiment of determination of KBr (g%) by volhard method In a flask; 15ml KBr was taken 25 ml 0.05M AgNO3 1 ml nitric acid 1 ml ferric alum indicator Then titration with 0.05M KSCN was done The end point was =15 ml Calculate the mass of KBr in g%
- The ascorbic acid, C,H;Os (176.124 g/mmol) content of a bottle of peach juice containing 2.50 L was determined by titration with a standard solution of potassium iodate, KIO3. The KIO; solution was prepared by dissolving 100.4 mg primary standard grade KIO; (214.001 mg/mmol) to a final volume of 250.0 mL. To a 200.00-mL aliquot of the sample, 10 mL of KI, 10 mL of HCl and 5 mL of starch solution were added and subsequently titrated, requiring 18.19 mL of the KIO; titrant. The relevant reactions are given below: KIO; + 5KI + 6H* → 3l2 + 6K* + 3H;0 CH;O, + l2→ CH,O, + 21- + 2H* a. How many millimoles of ascorbic acid is in the titrated sample? b. What is the mass of ascorbic acid per bottle of the peach juice?Part B Calculate the concentration of C,H,NH, HạOt, and OH- in a 0.225 M CH,NH Cl solution. (K (C,H,NH2) - 3.9 x 10-10) Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by commas. ? [C,H,NH,). H,O". JOH | = Submit Previous Answers Request AnswerWHAT VOLUME OF 0.107 N SILVER NITRATE IS REQUIRED TO TITRATE THE SODIUM CHLORIDE IN 4.0 G SAMPLE OF SODIUM LAURYL SULFATE? THE SAMPLE CLAIMS TO HAVE 6.8% NACL. WORKING FORMULA: %CONTENT = ((N X ML X MEQ)/WT.G) X 100
- of SCN 100 nt of dihted solution 2) If 5.0 mL of 0.00200 M Fe(NO3)3 is diluted to 50.0 mL, what is the concentration of Fe3+ in the diluted solution? Blank 0.00 M2-22. A 6.42% (w/w) Fe(NO,); (241.81 g/mol) solution has a density of 1.059 g/mL. Calculate (a) the molar analytical concentration of Fe(NO3)3 in this solution. (b) the mass in grams of Fe(NO;)3 in each liter of this solution.2.23 gr sample taken from a bleaching powder is dissolved and completed to 250 ml. Taken from here 25One ml of sample is titrated with 33.02 ml of 0.1158 N Na2S2O3 solution after the necessary procedures. Bleachingactive chlorine in powder (OClCalculate the amount and percentage. (OCl: 51.5 g / mol)