CATION CONFIRMATORY TEST OBSERVATION ADDED REAGENT(S) Excess NH3 KSCN K4Fe(CN)6 K3Fe(CN)6 Na₂C₂04 NaOH (in evaporating dish) ANION CONFIRMATORY TEST OBSERVATION ADDED REAGENT(S) HNO3, Fe(NO3)3 HNO3, KMnO4 (to the ppt) CH3COOH MgCl2 6M H₂SO4, FeSO4, 18M H₂SO4 POSSIBLE ION(S) PRESENT? OBSERVATIONS brown ppt Blood red complex Prussian blue ppt NVR NVR Litmus paper: red to blue OBSERVATIONS Yellow aqueous layer; pink toluene layer Yellow-brown aqueous layer; pink toluene layer N/A NVR NVR

2H+ + Na2CO3⟶2Na+ + H2O + CO2    the volume of 28.30 ± 0.06 mL of HNO3 solution was required for complete reaction with 0.8450 ± 0.0009 g of Na2CO3, (FM 105.988 ± 0.001 g/mol). Please Find the molarity of the HNO3 solution along with its absolute uncertainty. 1. [HNO3] = ________________ M 2. ___ ± ____________ M

please help me find average and standard deviation

i have hard time geting it stright even after I do the experiment can  u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…

Kk.343.

Blank determinations reveal errors due to interfering contaminants from the reaagents and vessels employed in the analysis.

Complete the table and provide the percent (%) recovery for each extraction.

A volume of 250 ml of a 0.05 M solution of a reagent of formula weight (relative molecular mass) 40 was made up, the weighing being done by difference. The standard deviation of each weighing was 0.0001 g. 1 (a) What were the standard deviation and relative standard deviation of the weight of reagent used?

A 10.00 mL of natural water sample containing Ni2+ was pipetted into a volumetric flask and diluted to 50.00 mL with pure water. In the second 10.00 mL of natural water sample transferred into a volumetric flask, exactly 4.00 mL of a Ni2+ solution with a concentration of 5.99 mg/L was added and then diluted to 50.00 mL with pure water. The measured absorbance is A1= 0.436 and A2 = 0.663. What is the Ni2+ concentration in unit of mg/L in the natural water sample?

Find the weight percent %Ca