Calculate the gravimetric factor for phosphate in KH2 PO4. Calculate the gravimetric factor for phosphate in KH2PO 4. 0.4706 0.5881 0.6570 0.6979 0.4119 0.2276 0.343(

1. A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer? 2. Data in the table below were collected at 25°C for the following reaction:2 I–(aq) + S2O82–(aq) I2 (aq) + 2 SO42-(aq) a) Determine the rate law for the reaction. b) Calculate the rate constant, giving the correct units for k.

A sample of material contains the components NaOH, Na2CO3, NaHCO3 , or possible mixtures of these. Two samples, each weighing 1 .000 gram, are dissolved in water. To one sample phenolphthalein is added and the solution is titrated cold with 1.038 N acid, of which 17.96 ml are required. The other sample is titrated cold with methyl orange as an indicator, and 21.17 ml of the same acid is required. Calculate the percentage of alkalies present.

Q/ Mohr's method uses the potassium chromate indicator and this indicator makes the equivalent point not identical to the end point. A sample weighing 5.592 g of BaCl2 is dissolved in 500 mL of water. Calculate the percentage of chloride in the sample when 25 mL of the sample is titrated and requires 33.47 mL of 0.1098 N AGNO. SOLUTION:

The accepted value of K is 1.2 x 10 -12 for AgCro, Calculate the percentage error if your experimentally determined value for K, was 1.4x 10 10

Can you please help me with a, b, c and d    A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4     a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer.  b)  Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer.  c)  Calculate the pH of the buffer solution.  d)  What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?

Calculate the enthalpy of solution (ΔH for the dissolution) per mole of NH4NO3 under the conditions described in the given problem.

A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10–4.   What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?

(c) What is a standard solution? What piece of glassware is used to prepare a standard solution and describe how a standard solution of sodium carbonate may be prepared in the laboratory?

g The solubility of Mg(OH)2 in water at 25 °C is measured to be 0.0096 Use this information to calculate K for Mg(OH)2. Round your answer to 2 significant digits. 00 L 3