A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 18.00 mL sample of her gastric juices and titrate the sample with 4.95 × 10-4 M KOH. The gastric juice sample required 4.58 mL of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. pH = Incorrect 4.9 For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia? no unable to determine yes
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Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration.
I got 4.9 and it says it's incorrect. What did I do wrong?
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- A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 18.00 mL sample of her gastric juices and titrate the sample with 4.85 × 10-4 M KOH. The gastric juice sample required 1.26 mL of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. pH = For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia? unable to determine no yesA patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 18.00 mL sample of her gastric juices and titrate the sample with 3.94 x 10-4 M KOH. The gastric juice sample required 6.60 mL of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. pH = Enter numeric value For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia? no O unable to determine O yesIn a hospital laboratory, a 10.0 mL sample of gastric juice, obtained several hours after a meal, was titrated with 0.01 M NaOH to neutral pH of 7.0; 72.0 mL of NaOH was required for this titration. The patient’s stomach contained no ingested food or drink, thus assume that no buffers were present. What was the pH of the 10.0 mL gastric juice sample before titrating with NaOH?
- A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units unitscalculate the amount of that food that you would need to ingest for it to be fatal to a human assuming there is a 5 l of blood in the human body is this an amount that you need to be concerned about? explain amount needed: 5ml Final pH: 5.8A mixture containing only KCl and NaBr is analyzed by the Mohr Method. A 0.3172-g sample is dissolved in 50 mL water and titrated to the Ag2CrO4 endpoint, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same endpoint. Report the % (w/w) KCl and NaBr in the sample. [Ans . 84.41 % (w /w); 17.59 % (w /w)]
- Consider a buffer solution of acetate. The volume is 500 ml, the concentration is 200 mM, and the pH is 5.0. a. How many total moles of acetate plus acetic acid are present in the solution? Express answer as x.y with one digit before and one after the decimal place. b. What is the ratio of acetate ions (Ac-) to acetic acid ions (HAc) in the buffer solution (pH 5.0) if the pka is 4.76? Express the answer as x.yz with one digit before and two after the decimal place. c. How many moles of acetate are present in the solution? Express your answer to one decimal place. d. How many moles of acetic acid are present in the solution? Express your answer to one decimal place.A patient is prescribed 0.151 g of Lidocaine intravenously. The lidocaine is available as a 12 mg/mL solution. How many mL must be administered?A sample was analysed for renal and liver function tests. The sample was from a 50-year- old man who had seen his GP to report problems with tiredness. The results observed were reviewed (reference ranges are given in brackets): Sodium Potassium Urea Creatinine Alkaline phosphatase Alanine aminotransferase Albumin Bilirubin Explain these results. 200 mmol/L >10 mmol/L 6.2 mmol/L 87 μmol/L 153 IU/L 34 IU/L 40 g/L 12 μmol/L (135-145) (3.5-5.0) (3.5-6.6) (70-150) (95-320) (5-42) (35-50) (<17)
- Refer to the titration curve in answering the questions: 13. 12 11 10 9 등 8 7 6 5 4 3 0 -~ 2 4 6 8 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Unknown Acid 0.10 mol/L - titrant = NaOH 0.1 mol/L 1. Which of the following is True in terms of the relative concentrations of analyte species for the unknown acid at pH 7.0? A. [H₂A] > [HA] B. [H3A]> [H₂A] C. [H₂A] <[HA] D. [HA] < [A] E. [H₂A] = [HA] 2. The value of the first equivalence point is equal to? 3. The value of the first pKA is? tenths) (answer must be in nearest 4. In the unknown acid above, how many ionizable protons are actually present? 5. An unknown acid in the figure above was titrated with 0.10 M of NaOH (titrant) (note: n is the number of ionizable protons) In the titration curve above, how many equivalence points are actually present?Absorbance of urea for a diabetic patient is 0.335 while 0.214 is the absorbance of standard kit for the same test, calculate the concentration of this test ? Concentration of standard kit = 50 mg/dl. Repl...You obtained the following raw data when setting up a Biuret standard curve: BSA (mg/ml) Absorbancy 540nm 0 0.158 1 0.210 2 0.260 3 0.305 4 0.360 5 0.410 6 0.455 7 0.510 8 0.530 9 0.550 10 0.554 After blanking against a biuret-dH2O sample, the protein concentration of an unknown sample was determined using the same method and an absorbancy of 0.262 was obtained. Set up a standard curve, excluding outliers (experimental and statistical) and determine the protein concentration in the unknown sample in mg / ml (up to 3 significant figures).