31. What is the solubility product expression for La(OH)3? a) K,= [La*][30H¯] K,= [La*][3OH¯}' K„=[La*+][OH¯]° c) %3D sp b) [La*(OH,)] 3+ [La**][OH¯] [La**(OH,)] %3D [La" ][OH] 3+ d) e) f) none of the above
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- The protein in a 0.2976 -g sample of cheese is determined by the Kjeldahl method. The sample is digested with H2SO4, the resulting solution made basic with NaOH, and the ammonia distilled into 50.00 mL of 0.09756 M HCl. The excess HCl is then back titrated using 39.87 mL of 0.05345 M NaOH. Calculate the % N and % protein of the sample.The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________Calculate the initial concentration of Fe3+, based on the dilution that results from adding KSCN solution and water to the original 0.0020 M Fe(NO3)3solution. See Step 2 of the procedure for the volume of each substance used in Test Tubes 1-4. This value will be the same value for all four test tubes. This is essentially the same as filling out part of the “I” row in an ICE table. Test tube number 0.0020 M Fe(NO3)3(mL) 0.0020M KSCN(mL) H2O(mL) 1 5 2 3 2 5 3 2 3 5 4 1 4 5 5 0
- A student performed an acid-base titration in the lab and recorded the results as shown below. Look very carefully at the results and answer the questions which follow. 7. 演定結果 21 3. 346 27.40 00 36 終結摘定管讀數(cm) 開始定管數(Cm 所需演定州的積(cm) 44 標 (a) Why do we perform acid-base titrations in our labs? (b) In the titration performed by the student, what was the net ionic equation for the chemical reaction occurring?The ICE table below shows the results of this experiment for one run of test tube 11. Note that the units of concentration are micromoles per liter! Fe3+ (µM) SCN- (uM) Fe(SCN)2* (µM) | 714 357 |C -X -X +X E 682 325 32 Calculate the value of K for the reaction based on this data. Use three significant digits in your answer. 0.0001The expression for the solubility product of Ca3(PO4)2 is: 2+1 3 2 [Ca²+]³ x [PO³ ]² 3- 4 2+ 3- 03 [Ca²+] × 2 [PO³-] 4 2+ 3 3 [Ca ²+1³ + 2[PO³ ]² 2 3- 4 3- 2 [3 × Ca²+]³ × [2 × PO³-]² 4
- Which of the following is the correct Ksp expression for the insoluble solid, Ag,SO,? A) K sp 2[Ag*][SO}¯] B) K sp = [Ag*][SO}¯] C) Ksp = [Ag*]*[SO?¯] [Ag*]*[SO?¯] D) K en = Ag,SO4 ds 2[Ag*][S0}¯] K sp E) Ag,sO4 A) see problem image A) B) see problem image B) C) see problem image C) D) see problem image D) E) see problem image E)As part of the analysis of water samples, the hardness of water is commonly measured and calculated. It is commonly expressed in ppm by mass (parts per million) of CaCO3. Parts per million is also equivalent to milligrams of CACO3 per liter of water. In a sample taken by an environmentalist, he was able to observe a hardness count of 205 mg CacO3/L. Given this hardness count of the sample, what is the molar concentration of Ca2+ ions in the water sample?Complete the following solubility constant expression for PbCO3. K = 0 sp X 00 S
- TRAG 722 2 5. Enough NaCN was added to 0.030 M silver nitrate (AgNO3) to give a solution that was initially 0.460 Ma cyanide ion (CN-). What is the concentration of silver ion (Ag*) in this solution after Ag(CN)₂ forms? Kr for Ag(CN)2 is 5.6 x10¹8Addition of an excess silver nitrate to a 0.5012 g sample yielded a mixture of AgCl and Agl that weighed 0.4700 g. The precipitate was then heated in a stream of Cl2 to convert the Agl to AgCl. 2 Agl (s) + Cl2 (g) 2 AgCI (s) + 12(g) The precipitate was found to weigh 0.3900 g after this treatment. Calculate the percentages of NH4I and NH4CI, respectively. 19.71, 25.07 25.07, 28.72 28.72, 19.95 O 25.07, 19.71 O 19.95, 28.72Try Again Check your exponents. Write the concentration equilibrium constant expression for this reaction. 3 1₂(s) + 2 Cr³+ (aq) + 7 H₂O(1)→ Cr₂O² (aq) +61¯ (aq) + 14 H* (aq) [₂0][₁][H]¹⁹ 3+ [¹] Η + 19 X Ś 00