1 A 67.0 ml, 0.220 M calcium nitrate solution is mixed with 95.0 mL of 0.130 M ammonium nitrate solution. Calculate the concentrations (with units of M) of all ionic species in the finalsolution.[NO,]0.2582 M[NH*] = 0. 0762 M[Ca2+] = 0.0909 MSubmit Answer Submission not graded. Use fewer digits. Tries 0/10 Previous TriesThreaded View Chronological View Sorting/Filtering options Export? Preferences on what is marked as NEWMark NEW posts no longer newNEWAnonymous 1 Reply (Sun Oct 6 11:49:08 pm 2019 (CDT))It would be nice if you could submit answers individually.-Use fewer digits*Uses fewer digits*-Use mordigits*visible confusionWhat gives?NEWRania Chemrar (20CHEMRAR192191:brandonu) Reply (Sun Oct 11 09:14:48 pm 2020 (CDT))Only NH4+ needs more digitsEWRe: Anonymous 3 Reply (Sun Oct 11 09:47:54 pm 2020 (CDT))It's not accepting my answer :(P Type here to searchВ.2:34 AM4°C A 4) ENG2021-10-12% NTSCExperts please look into this question again.Thanks for all your efforts. keeps saying theanswer is wrong. Really tired of solving it.

Answered: Image /qna-images/answer/0057584b-3d77-43f1-9370-1846e9e41be0.jpg

A 67.0 ml, 0.220 M calcium nitrate solution is mixed with 95.0 mL of 0.130 M ammonium nitrate solution. Calculate the concentrations (with units of M) of all ionic species in the final solution. [NO, -0.2582 M [NH,"1=0. 0762 M |Ca+ 0.0909 M Submit Answer Submission not graded. Use fewer digits. Tries 0/10 Previnus Tries

A 67.0 ml, 0.220 M calcium nitrate solution is mixed with 95.0 mL of 0.130 M ammonium nitrate solution. Calculate the concentrations (with units of M) of all ionic species in the final solution. [NO, -0.2582 M [NH,"1=0. 0762 M |Ca+ 0.0909 M Submit Answer Submission not graded. Use fewer digits. Tries 0/10 Previnus Tries

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 95AP: 95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated...

See similar textbooks

Similar questions

Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1795 M0.1795 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 16.73 mL16.73 mL of the standard solution. What is the concentration of the original sulfuric acid solution?
We did a lab and have to answer the following question: What was the concentration of the NaOH solution? Show your calculations. If you did not use all of your data, explain why. This is the data that was obtained by the lab during 3 trials: KHP masses (g) --> 1 2 3 0.61 .061 0.65 Titration of KHP Run 1 Run 2 Run 3 original volume 40.20 mL 40.10 mL 40.20 mL final volume 6.89 mL 0.00 mL 0.00 mL volume used (final-initial) 33.31 mL 40.10 mL 40.20 mL concentration of NaOH (M) avg: concentration of NaOH (M) : also, should the values for volume used be negative or are they correct as is? And I'm not sure how to find the concentration from the values my lab group and I got.
A 0.9600 M NaOH solution was diluted with a factor of 4.Then the diluted solution of NaOH was titrated against an unknown acid.The volumes of NaOH(aq) titrated are shown in the table below.Volumes of NaOH(aq):RoughtitrationFirsttitrationSecondtitrationThirdtitrationThirdtitrationFinal burette reading:(mL)19.00 34.05 20.86 36.01 23.57Initial burette reading:(mL)19.00 19.07 5.76 21.02 8.54The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used ineach titration is 14.80 mL.(i) Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations andreasoning.(ii) What type of chemical reaction is this? _________________ or _______________
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
In a titration, 15.5 g of oxalic acid was dissolved in a flask and neutralized with 31.2 mL of NaOH. Determine the molarity of the NaOH. Hint: Primary standards (like oxalic acid, here) incude water in their formula. As a result, they do not absorb atmospheric water. Oxalic acid has the chemcial formula: H2C2O4⋅2H2O (so be sure to include the 2 extra water molecules). a. 8.33 M b. 3.55 M c. 7.88 mol/L d. 0.333 mol/L
Chemistry A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.100 g of this sample requires 23.98 mL of 0.100 M HCl . An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample? Express your answer to three significant figures and include the appropriate units.
A 25.0mL acetic acid sample was titrated using exactly 69.72 mL of a 0.30M sodium hydroxide solution until the endpoint was achieved. What is the molar concentration of the acid sample? A. 0.02 M B. 0.98 M C. 1.95 M D. 3.90 M E. 9.76 M
1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.
You collected the following data from a titration experiment using a 0.129M standardized NaOH solution to titrate a 26.55 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Trial 1 0.44 19.69 ?? Trial 2 0.18 17.2 Trial 3 0.50 19.94 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units.
A 25.00 mL sample of a vinegar solution is diluted to 250.00 mL with water. Then a 25.00 mL aliquot of the diluted sample is titrated with strong base, requiring 22.13 mL of 0.1027 M sodium hydroxide to reach the endpoint. What is the molar concentration of acetic acid in the original sample of vinegar before the dilution?(a) 2.278×10‒3 M(b) 2.278×10‒2 M(c) 0.09091 M(d) 0.9091 M